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1  Vol.  Post  8w,,  Illustrated.     New  York,  1851.     $1 
Sent  free  of  carriage  on  receipt  of  the  price. 

H,  BAILLIEEE,  290  Broadway, 


NEW  YORK, 


SYSTEM  OF   INSTRUCTION 


THE  PRACTICAL   USE 


THE  BLOWPIPE 


GRADUATED  COURSE  OF  ANALYSIS  FOR  THE  USE  OF  STUDENTS 

AND     ALL     THOSE     ENGAGED     IN     THE     EXAMINATION     OF 
METALLIC      COMBINATIONS. 


NEW    YOKE: 
II.    BAIL  LIE  RE,    290    BROADWAY, 

AND  219  REGENT  STREET,  LONDON. 

PARIS:    J.   B.   BAILLIERE    ET  TILS,    RUE    H  A  U  T  EFE  UILLE, 
MADRID :   C.  BAILLY-BAILLI&RE,  CALLE  DEL  PRINCIPE. 

1858. 


ENTBRRD  according  to  Act  of  Congress,  in  the  year  1858,  by 

C.   E.    B  AILLIERE, 
In  the  Clerk's  Office  of  the  District  Court  of  the  United  States,  for  the  Southern  District  of  New  York. 


W.  H.  TINSON,  Prii 


inA  StereOtyper,  43  Centre  Street. 


TABLE    OF    CONTENTS. 


PART   I. 


PAGE 

7 


Preface,     .  

The  Use  of  the  Blowpipe,  .....•••• 

Utensils— The  Blowpipe, 12 

The  Oil  Lamp, 22 

The  Spirit  Lamp, 23 

Charcoal  Support 24: 

Plntinum  Supports, 2^ 

Iron  Spoons, 28 

Glass  Tubes, 28 

Other  Apparatus  necessary, 31 

THE  REAGENTS, 34 

Reagents  of  General  Uso, 34 

Carbonate  of  Soda, 34 

Hydrate  of  Baryta, 35 

Bi-sulphate  of  Potassa, 35 

Oxalatc  of  Potassa,    .        .        .        .  •  •        .36 

Cyanide  of  Potassium, 36 

256295 


iv  CONTENTS. 

THE  REAGENTS  —  (continued.) 

Nitrate  of  Potassa, ,37 

Borax, 38 

Microcosmic  Salt, ,39 

Nitrate  of  Cobalt, .40 

Tin, 41 

Silica, 42 

Test  Papers,       .  .......     42 

ESPECIAL  REAGENTS, .43 

Boracic  Acid, 43 

Fluorspar, 43 

Oxalate  of  Nickel, 43 

Oxide  of  Copper, 43 

Antimoniate  of  Potassa, 44 

Silver  Foil, .44 

Nitroprusside  of  Sodium, ,44 


PART    II. 

Initiatory  Analysis, 47 

Examination  with  the  Glass  Bulb,      .......     47 

"  in  the  Open  Tube, 52 

"  upon  Charcoal, 55 

in  the  Platinum  Forceps,       .         .         .         .         .         .01 

in  the  Borax  Bead, <•>»•» 

in  Microcosmic  Salt,      .    *  .         .         .         .  70 

Table  I. — Colors  of  Beads  of  Borax  and  Microcosmic  Salt,        .         .75 
Table  II. — Behavior  of  Metallic  Oxydes  with  Borax  and  Microcosmic 

Salt, 85 

Examinations  with  Carbonate  of  Soda, 103 


C  O  N  T  K  NTS. 


PART    III- 

PAGE 

Special  Reactions, *' 

A. — METALLIC  OXIDES  : 

First  Group.— The   Alkalies:    Potassa,    Soda,  Ammonia,   and 

Lithia, 110 

Second  Group.— The  Alkaline  Earths :    Baryta,  Strontia,  Lime, 

and  Magnesia, Uo 

Third  Group.— The  Earths:  Alumina,  Gluciua,  Yttria,  Thorina, 

and  Zirconia, 1 

Fourth  Group.— Cerium,  Lanthanium,  Didymium,  Columbium, 
Niobium,  Pelopium,  Titanium,  Uranium,  Vanadium,  Chro 
mium,  Manganese, 1>2i 

Fifth  Group.— Iron,  Cobalt,  Nickel, 135 

Sixth  Group.— Zinc,  Cadmium,  Antimony,  Tellurium,          .         .  140 
Seventh  Group. — Lead,  Bismuth,  Tin, 

Eighth  Group.— Mercury,  Arsenic, .157 

Ninth  Group.— Copper,  Silver,  Gold, 161 

Tenth  Group. — Molybdenum,  Osmium,        .                  ...  165 
Eleventh  Group.— Platinum,  Palladium,  Iridium,  Rhodium,  Ru 
thenium,          167 

Non-Metallic  Substances, 168 

Tabular  Statement  of  the  Reactions  of  Minerals  before  the  Blowpipe,   178 
Carbon  and  Organic  Minerals,     ....        ..  -       •         •  181 

Potassa, _;    •         •         •  184 

Soda, 186 

Baryta  and  Strontia, 19<) 

Lime,          , 192 

Magnesia, '  .         .         .  196 

Alumina, 20() 

Silicates, 2u4 


vi  CON  T  E  NTS. 

PAQK 

Tabular  Statement,  etc. — (continued.) 

Uranium, 212 

Iron, 214 

Manganese, 222 

Nickel  and  Cobalt, 226 

Zinc, 232 

Bismuth, 234 

Lead, 238 

Copper, .         .  248 

Antimony, .•••-•  256 

Arsenic, 260 

Mercury, 262 

Silver,  264 


PREFACE. 


IT  is  believed  the  arrangement  of  the  present  work  is  superior 
to  that  of  many  of  its  predecessors,  as  a  vehicle  for  the  facili 
tation  of  the  student's  progress.  While  it  does  not  pretend  to 
any  other  rank  than  as  an  introduction  to  the  larger  works,  it 
is  hoped  that  the  arrangement  of  its  matter  is  such  that  the 
beginner  may  more  readily  comprehend  the  entire  subject  of 
Blowpipe  Analysis  than  if  he  were  to  begin  his  studies  by  the 
perusal  of  the  more  copious  works  of  Berzelius  and  Plattner. 

When  the  student  shall  have  gone  through  these  pages,  and 
repeated  the  various  reactions  described,  then  he  will  be  fully 
prepared  to  enter  upon  the  study  of  the  larger  works.  To 
progress  through  them  will  then  be  but  a  comparatively  easy 
task. 

The  arrangement  of  this  little  work  has  been  such  as  the 
author  and  his  friends  have  considered  the  best  that  could  be 
devised  for  the  purpose  of  facilitating  the  progress  of  the 


yjii  PREFACE. 

student.  Whether  we  have  succeeded  is  left  for  the  public  to 
decide.  The  author  is  indebted  to  several  of  his  friends  for 
valuable  contributions  and  suggestions. 

S. 
CINCINNATI,  June,  1857. 


THE     BLOWPIPE. 


Part   First. 


9 

THE   USE   OF   THE   BLOWPIPE. 

PERHAPS  during  the  last  fifty  years,  no  department  of  chem 
istry  has  been  so  enriched  as  that  relating  to  analysis  by  means 
of  the  Blowpipe. 

Through  the  unwearied  exertions  of  men  of  science,  the  use 
of  this  instrument  has  arrived  to  such  a  degree  of  perfection, 
that  we  have  a  right  to  term  its  use,  "  Analysis  in  the  dry 
way/'  in  contradistinction  to  analysis  "in  the  wet  way."  The 
manipulations  are  so  simple  and  expeditious,  and  the  results  so 
clear  and  characteristic,  that  the  Blowpipe  analysis  not  only 
verifies  and  completes  the  results  of  analysis  in  the  wet  way, 
but  it  gives  in  many  cases  direct  evidences  of  the  presence  or 
absence  of  many  substances,  which  would  not  be  otherwise 
detected,  but  through  a  troublesome  and  tedjous  process? 
involving  both  -prolixity  and  time  ;  for  instance,  the  detection 
of  manganese  in  minerals. 

Many  substances  have  to  go  through  Blowpipe  manipulations 
before  they  can  be  submitted  to  an  analysis  in  the  wet  way, 

1* 


10      t{°,  •  «/£    ;  :T  H;  E     B.'i,  o  \y  P  i  r  E  . 

The  apparatus  and  reagents  employed  are  compendious  and 
small  in  number,  so  that  they  can  be  carried  easily  while  on 
scientific  excursions,  a  considerable  advantage  for  mineralogists 
and  metallurgists. 

The  principal  operations  with  the  Blowpipe  may  be  ex 
plained  briefly  as  follows  : 

(a.)  By  Ignition  is  meant  the  exposure  of  a  substance  to 
such  a  degree  of  heat,  that  it  glows  or  emits  light,  or  becomes 
red-hot.  Its  greatest  value  is  in  the  separation  of  a  volatile 
substance  from  one  less  volatile,  or  one  which  is  entirely  fixed 
at  the  temperature  of  the  flame.  In  this  case  we  only  take 
cognizance  of  the  latter  or  fixed  substance,  although  in  many 
instances  we  make  use  of  ignition  for  the  purpose  of  changing 
the  conditions  of  a  substance,  for  example,  the  sesqui-oxide 
of  chromium  (Cr203)  in  its  insoluble  modification  ;  and  as  a 
preliminary  examination  fqr  the  purpose  of  ascertaining  whether 
the  subject  of  inquiry  be  a  combination  of  an  organic  or  inor 
ganic  nature. 

The  apparatus  used  for  this  purpose  are  crucibles  of  pla 
tinum  or  silver,  platinum  foil,  a  platinum  spoon,  platinum  wire 
or  tongs,  charcoal,  glass  tubes,  and  iron  spoons. 

(&.)  Sublimation  is  that  process  by  which  we  convert  a  solid 
substance  into  vapor  by  means  of  a  strong  heat.  These  vapors 
are  condensed  by  refrigeration  into  the  solid  form.  It  may  be 
termed  a  distillation  of  a  solid  substance.  Sublimation  is  of 
great  consequence  in  the  detection  of  many  substances  ;  for 
nstance,  arsenic,  antimony,  mercury,  etc. 

The  apparatus  used  for  the  purposes  of  sublimation  consist 
of  glass  tubes  closed  at  one  end. 

(c.)  Fusion. — Many  substances  when  exposed  to  a  certain 
degree  of  heat  lose  their  solid  form,  and  are  converted  into 
a  liquid.  Those  substances  which  do  not  become  converted 
into  the  liquid  state  by  heat,  are  said  to  be  infusible.  It  is  a 
convenient  classification  to  arrange  substances  into  those  which 
are  fusible  with  difficulty,  and  those  which  are  easily  fusible. 
Very  often  we  resort  to  fusion  for  the  purpose  of  decomposing  a 


1  T  8       U  S  E  .  11 

substance,  or  to  cause  it  to  enter  into  other  combinations,  by 
which  means  it  is  the  more  readily  detected.  If  insoluble  sub 
stances  are  fused  with  others  more  fusible  (reagents)  for  the 
purpose  of  causing  a  combination  which  is  soluble  in  water  and 
acids,  the  operation  is  termed  unch  ting.  These  substances  are 
particularly  the  silicates  andthe  sulphates  of  the  alkaline 
earths.  The  usual  reagents  resorted  to  for  this  purpose  are 
carbonate  of  soda  (NaO,  CO2),  carbonate  of  potash  (KO, 
CO3),  or  still  better,  a  mixture  of  the  two  in  equal  parts.  In 
some  cases  we  use  the  hydrate  of  barytes  (BaO,  HO)  and  the 
bisulphate  of  potash  (KO,  2S03).  The  platinum  spoon  is 
generally  used  for  this  manipulation. 

Substances  are  exposed  to  fusion  for  the  purpose  of  getting 
a  new  combination  which  has  such  distinctive  characteristics 
that  we  can  class  it  under  a  certain  group  ;  or  for  the  purpose 
of  ascertaining  at  once  what  the  substance  may  be.  The  re 
agents  used  for  this  purpose  are  borax  (NaO,  2Br03)  and 
the  microcosmic  salt  (NaO,  NIPO,  PO5,  HO).  Charcoal 
and  the  platinum  wire  are  used  as  supports  for  this  kind  of 
operation. 

(d.)  Oxidation. — The  chemical  combination  of  any  substance 
with  oxygen  is  termed  oxidation,  and  the  products  are  termed 
oxides.  As  these  oxides  have  qualities  differing  from  those 
which  are  non-oxidized,  it  therefore  frequently  becomes  neces 
sary  to  convert  substances  into'  oxides  ;  or,  if  they  are  such, 
of  a  lower  degree,  to  convert  them  into  a  higher  degree  of 
oxidation.  These  different  states  of  oxidation  frequently  pre 
sent  characteristic  marks  of  identity  sufficient  to  enable  us  to 
draw  conclusions  in  relation  to  the  substance  under  examina 
tion.  For  instance,  the  oxidation  of  manganese,  of  arsenic,  etc. 
The  conditions  necessary  for  oxidation,  are  high  temperature 
and  the  free  admission  of  air  to  the  substance. 

If  the  oxidation  is  effected  through  the  addition  of  a  sub 
stance  containing  oxygen  (for  instance,  the  nitrate  or  chlorate 
of  potash)  and  the  heating  is  accompanied  by  a  lively  defla 
gration  and  crackling  noise,  it  is  termed  detonation.  By  this 


12  THE     BLOWPIPE. 

process  we  frequently  effect  the  oxidation  of  a  substance,  and 
thus  we  prove  the  presence  or  the  absence  of  a  certain  class 
of  substances.  For  instance,  if  we  detonate  (as  it  is  termed 
by  the  German  chemists)  the  sulphide  of  antimony,  or  the 
sulphide  of  arsenic  with  nitrate  of  potash,  we  get  the  nitrate 
of  antimony,  or  the  nitrate  of  arsenic.  The  salts  of  nitric  or 
chloric  acid  are  determined  by  fusing  them  with  the  cyanide 
of  potassium,  because  the  salts  of  these  acids  detonate. 

(e.)  Reduction. — If  we  deprive  an  oxidized  substance  of  its 
oxygen,  we  term  the  process  reduction.  This  is  effected  by 
fusing  the  substance  under  examination  with  another  which 
possesses  a  greater  affinity  for  oxygen.  The  agents  used 
for  reduction  are  hydrogen,  charcoal,  soda,  cyanide  of  potas 
sium,  etc.  Substances  generally,  when  in  the  unoxidized  state, 
have  such  characteristic  qualities,  that  they  cannot  very  readily 
be  mistaken  for  others.  For  this  reason,  reduction  is  a  very 
excellent  expedient  for  the  purpose  of  discerning  and  classifying 
many  substances. 


B.    UTENSILS. 

We  shall  give  here  a  brief  description  of  the  most  necessary 
apparatus  used  for  analysis  in  the  dry  way,  and  of  their  use. 

The  Blowpipe  is  a  small  instrument,  made  generally  out  of 
brass,  silver,  or  German  silver,  and  was  principally  used  in  ear 
lier  times  for  the  purpose  of  soldering  small  pieces  of  metals 
together.  It  is  generally  made  in  the  form  of  a  tube,  bent  at 
a  right  angle,  buj;jy^thpi;it_j^  The  largest  one  is 

about  seven  inches  long,  and  the  smallest  about  two  inches. 
The  latter  one  terminates  with  a  small  point,  with  a  small 
orifice.  The  first  use  of  the  blowpipe  that  we  have  recorded 
is  that  of  a  Swedish  mining  officer,  who  used  it  in  the  year  1738 
for  chemical  purposes,  but  we  have  the  most  meagre  accounts 
of  his  operations.  In  1158  another  Swedish  mining  officer,  by 
the  name  of  Cronstedt,  published  his  "  Use  of  the  Blowpipe  in 


ITS     USE. 


13 


Chemistry  and  Mineralogy,"  translated  into  English,  in  1170, 
by  Van  Engestroem.  Bergman  extended  its  use,  and  after 
him  Ghan  arid  the  venerable  Berzelius 
a  *  -((1S21).  The  blowpipe  most  generally 
used  in  chemical  examinations  is  com 
posed  of  the  following  parts  :  (Fig.  1.) 
A  is  a  little  reservoir  made  aigjjgbt  by 
grinding  the  part  B  into  it.  This  re 
servoir  serves  the  purpose  of  retaining 
the  moisture  with  which  the  air  from 
the  mouth  is  charged.  A  small  coni 
cal  tube  is  fitted  to  this  reservoir. 
This  tube  terminates  in  a  fine  ori 
fice.  As  this  small  point  is  liable  to 
get  clogged  up  with  soot,  etc.,  it  is  bet 
ter  that  it  should  be  made  of  platinum, 
so  that  it  may  be  ignited.  Two  of 
these  platinum  tubes  should  be  supplied, 
differing  in  the  size  of  the  orifice,  by 
which  a  stronger  or  lighter  current 
of  flame  may  be  projected  from  it. 
Metals,  such  as  brass  or  German  sil 
ver,  are  very  liable  to  become  dirty 
through  oxidation,  and  when  placed 
between  the  lips  are  liable  to  im 
part  a  disagreeable  taste.  To  avoid 
this,  the  top  of  the  tube  must  be  sup 
plied  with  a  mouthpiece  of  ivory 
or  horn  C.  The  blowpipe  here  repre 
sented  is  the  one  used  by  Ghan,  and 
approved  by  Berzelius.  The  trumpet  mouthpiece  was  adopted 
by  Plattner ;  it  is  pressed  upon  the  lips  while  blowing,  which 
is  less  tiresome  than  holding  the  mouthpiece  between  the  lips, 
although  many  prefer  the  latter  mode. 

Dr.  Black's  blowpipe  is  as  good  an  instrument  and  cheaper. 


14  THE     BLOWPIPE. 

It  consists  of  two  tubes,  soldered  at  a  right  angle  ;  the  larger 
one,  into  which  the  air  is  blown,  is  of  sufficient  capacity  to 
serve  as  a  reservoir. 

A  chemist  can,  with  a  blowpipe  and  a  piece  of  charcoal, 
determine  many  substances  without  any  reagents,  thus  enabling 
him,  even  when  travelling,  to  make  useful  investigations  with 
means  which  are  always  at  his  disposal.  There  are  pocket 
blowpipes  as  portable  as  a  pencil  case,  such  as  Wollaston's 
and  Mitscherlich's  ;  these  are  objectionable  for  continued 
use  as  their  construction  requires  the  use  of  a  metallic 
mouthpiece.  Mr.  Casamajor,  of  New  York,  has  made  one 
lately  which  has  an  ivory  mouthpiece,  and  which,  when  in  use, 
is  like  Dr.  Black's. 

The  length  of  the  blowpipe  is  generally  seven  or  eight 
inches,  but  this  depends  very  much  upon  the  visual  angle  of 


the    operators.      A   short-sighted    person,    of   course,    would 


I  T  S       U  8  E  .  15 

require  an  instrument  of  less  length  than  would  suit  a  far- 
sighted  person. 

The  purpose  required  of  the  blowpipe  is  to  introduce  a  fine 
current  of  air  into  the  flame  of  a  candle  or  lamp,  by  which  a 
higher  degree  of  heat  is  induced,  and  consequently  combustion 
is  more  rapidly  accomplished. 

By  inspecting  the  flame  of  a  candle  burning  under  usual 
circumstances,  we  perceive  at  the  bottom  of  the  flame  a  por 
tion  which  is  of  a  light  blue  color  (a  b),  Fig.  2,  which  gra 
dually  diminishes  in  size  as  it  recedes  from  the  wick,  and  disap 
pears  when  it  reaches  the  perpendicular  side  of  the  flame.  In 
the  midst  of  the  flame  there  is  a  dark  nucleus  with  a  conical 
form  (c).  This  is  enveloped  by  the  illuminating  portion  of  the 
flame  (d).  At  the  exterior  edge  of  the  part  d  we  perceive  a 
thin,  scarcely  visible  veil,  a,  e,  c,  which  is  broader  near  the 
apex  of  the  flame.  The  action  of  the  burning  candle  may  be 
thus  explained.  The  radiant  heat  from  the  flame  melts  the 
tallow  or  wax,  which  then  passes  up  into  the  texture  of  the 
wick  by  capillary  attraction  until  it  reaches  the  glowing  wick, 
where  the  heat  decomposes  the  combustible  matter  into  carbo 
nated  hydrogen  (C4H4),  and  into  carbonic  oxide  (CO). 

While  these  gases  are  rising  in  hot  condition,  the  air  comes 
in  contact  with  them  and  effects  their  combustion.  The  dark 
portion,  c,  of  the  flame  is  where  the  carbon  and  gases  have  not 
a  sufficiency  of  air  for  their  thorough  combustion  ;  but  gra 
dually  they  become  mixed  with  air,  although  not  then  sufficient 
for  complete  combustion.  The  hydrogen  is  first  oxidized  or 
burnt,  and  then  the  carbon  is  attacked  by  the  air,  although  par 
ticles  of  carbon  are  separated,  and  it  is  these,  in  a  state  of 
intense  ignition,  which  produce  the  illumination.  By  bringing 
any  oxidizable  substance  into  this  portion  of  the  flame,  it  oxi 
dizes  very  quickly  in  consequence  of  the  high  temperature  and 
the  free  access  of  air.  For  that  reason  this  part  of  the 
flame  is  termed  the  oxidizing  flame,  while  the  illuminating  por 
tion,  by  its  tendency  to  abstract  oxygen  for  the  purpose  of 
complete  combustion,  easily  reduces  oxidated  substances 


16  THE     BLOW  PIPE. 

brought  into  it,  and  it  is,  therefore,  called  the  flame  of  reduc 
tion.  In  the  oxidizing  flama,  on  the  contrary,  all  the  carbon 
which  exists  in  the  interior  of  the  flame  is  oxidized  into 
carbonic  acid  (CO2)  and  carbonic  oxide  (GO),  while  the 
blue  color  of  the  cone  of  the  flame  is  caused  by  the  complete 
combustion  of  the  carbonic  oxide.  These  two  portions  of  the 
flame — the  oxidizing  and  the  reducing — are  the  principal 
agents  of  blowpipe  analysis. 

If  we  introduce  a  fine  current  of  air  into  a  flame,  we  notice 
the  following  :  The  air  strikes  first  the  dark  nucleus,  and  forc 
ing  the  gases  beyond  it,  mixes  with  them,  by  which  oxygen  is 
mingled  freely  with  them.  This  effects  the  complete  combus 
tion  of  the  gases  at  a  certain  distance  from  the  point  of  the 
blowpipe.  At  this  place  the  flame  has  the  highest  tempera 
ture,  forming  there  the  point  of  a  b,ue  cone.  The  illuminated 
or  reducing  portion  of  the  flame  is  enveloped  outside  and 
inside  by  a  very  hot  flame,  whereby  its  own  temperature  is  so 
much  increased  that  in  this  reduction-flame  many  substances 
will  undergo  fusion  which  would  prove  perfectly  refractory  in 
a  common  flame.  Tiie  exterior  scarcely  visible  part  loses  its 
form,  is  diminished,  and  pressed  more  to  a  point,  by  which  its 
heating  power  is  greatly  increased. 

The  Blast  of  Air. — By  using  the  blowpipe  for  chemical  pur 
poses,  the  effect  intended  to  be  produced  is  an  uninterrupted 
steady  stream  of  air  for  many  minutes  together,  if  necessary, 
without  an  instant's  cessation.  Therefore,  the  blowing  can 
only  be  effected  with  the  muscles  of  the  cheeks,  and  not  by  the 
exertion  of  the  lungs.  It  is  only  by  this  means  that  a  steady 
constant  stream  of  air  can  be  kept  up,  while  the  lungs  will  not 
be  injured  by  the  deprival  of  air.  The  details  of  the  pro 
per  manner  of  using  the  blowpipe  are  really  more  difficult  to 
describe  than  to  acquire  by  practice  ;  therefore  the  pupil  is 
requested  to  apply  himself  at  once  to  its  practice,  by  which  he 
will  soon  learn  to  produce  a  steady  current  of  air,  and  to  dis 
tinguish  the  different  flames  from  each  other.  We  would 
simply  say  that  the  tongue  must  be  applied  to  the  roof  of  the 


1  T  8      U  8  K  .  IT 

inouth,  so  as  to  interrupt  the  coinmuuicatiou  between  the 
passage  of  the  nostrils  and  the  inouth.  The  operator  now  fills 
his  mouth  with  air,  which  is  to  be  passed  through  the  pipe  by 
compressing  the  muscles  of  the  cheeks,  while  he  breathes 
through  the  nostrils,  and  uses  the  palate  as  a  valve.  When 
the  mouth  becomes  nearly  empty,  it  is  replenished  by  the 
lungs  in  an  instant,  while  the  tongue  is  momentarily  withdrawn 
from  the  roof  of  the  mouth.  The  stream  of  air  can  be  continued 
for  a  long  time,  without  the  least  fatigue  or  injury  to  the  lungs. 
The  easiest  way  for  the  student  to  accustom  himself  to  the 
use  of  the  blowpipe,  is  first  to  learn  to  fill  the  mouth  with  air, 
and  while  the  lips  are  kept  firmly  closed  to  breathe  freely  through 
the  nostrils.  Having  effected  this  much,  he  may  introduce  the 
mouthpiece  of  the  blowpipe  between  his  lips.  By  inflating  the 
cheeks,  and  breathing  through  the  nostrils,  he  will  soon  learn 
to  *se  the  instrument  without  the  least  fatigue.  The  air  is 
forced  through  the  tube  against  the  flame  by  the  action  of  the 
muscles  of  the  cheeks,  while  he  continues  to  breathe  without 
interruption  through  the  nostrils.  Having  become  acquainted 
with  this  process,  it  only  requires  some  practice  to  produce  a 
steady  jet  of  flame.  A  defect  in  the  nature  of  the  combustible 
used,  as  bad  oil,  such  as  fish  oil,  or  oil  thickened  by  long  stand 
ing  or  by  dirt,  dirty  cotton  wick,  or  an  untrimmed  one,  or  a 
dirty  wickholder,  or  a  want  of  steadiness  of  the  hand  that 
holds  the  blowpipe,  will  prevent  a  steady  jet  of  flame.  But 
frequently  the  fault  lies  in  the  orifice  of  the  jet,  or  too  smrall 
a  hole,  or  its  partial  stoppage  by  dirt,  which  will  prevent  a 
steady  jet  of  air,  and  lead  to  difficulty.  With  a  good  blowpipe 
the  air  projects  the  entire  flame,  forming  a  horizontal,  blue 
cone  of  flame,  which  converges  to  a  point  at  about  an  inch  from 
the  wick,  with  a  larger,  longer,  and  more  luminous  flame 
enveloping  it,  and  terminating  to  a  point  beyond  that  of  the 
blue  flame. 

To  produce  an  efficient  flame  of  oxidation,  put  the  point 
of  the  blowpipe  into  the  flame  about  one  third  the  diameter 
of  the  wick,  and  about  one  twelfth  of  an  inch  above  it.  This, 


18 


THE     BLOWPIPE. 


however,  depends  upon  the  size  of  the  flame  used.  Blow  strong 
enough  to  keep  the  flame  straight  and  horizontal,  using  the 
largest  orifice  for  the  purpose.  Upon  examining  the  flame 
thus  produced,  we  will  observe  a  long,  blue  flame,  a  5,  Fig.  3, 
which  letters  correspond  with  the  same  letters  in  Fig.  2.  But 
this  flame  has  changed  its  form,  and  contains  all  the  combus 
tible  gases.  It  forms  now  a  thin,  blue  cone,  which  converges 
to  a  point  about  an  inch  from  the  wick.  This  point  of  the 


flame  possesses  the  highest  intensity  of  temperature,  for  there 
the  combustion  of  the  gases  is  the  most  complete.  In  the 
original  flame,  the  hottest  part  forms  the  external  envelope, 
but  here  it  is  compressed  more  into  a  point,  forming  the  cone 
of  the  blue  flame,  and  likewise  an  envelope  of  flame  surround 
ing  the  blue  one,  extending  beyond  it  from  a  to  c,  and  present 
ing  a  light  bluish  or  brownish  color.  The  external  flame  has 
the  highest  temperature  at  d,  but  this  decreases  from  d  to  c. 

If  there  is  a  very  high  temperature,  the  oxidation  is  not 
effected  so  readily  in  many  cases,  unless  the  substance  is  removed 
a  little  from  the  flame  ;  but  if  the  heat  be  not  too  high,  it  is 
readily  oxidized  in  the  flame,  or  near  its  cone,  If  the  current 


I  T  S       U  8  E  .  19 

of  air  is  blown  too  freely  or  violently  into  the  flame,  more  air  is 
forced  there  than  is  sufficient  to  consume  the  gases.  This 
superfluous  air  only  acts  detrimentally,  by  cooling  the  flame. 

In  general  the  operation  proceeds  best  when  the  substance  is 
kept  at  a  dull  red  heat.  The  blue  cone  must  be  kept  free  from 
straggling  rays  of  the  yellow  or  reduction  flame.  If  the  analy 
sis  be  effected  on  charcoal,  the  blast  should  not  be  too  strong, 
as  a  part  of  the  coal  would  be  converted  into  carbonic  oxide, 
which  would  act  antagonistically  to  the  oxidation.  The  oxida 
tion  flame  requires  a  steady  current  of  air,  for  the  purpose  of 
keeping  the  blue  cone  constantly  of  the  same  length.  For  the 
purpose  of  acquiring  practice,  the  following  may  be  done  : 
Melt  a  little  molybdeuic  acid  with  some  borax,  upon  a  platinum 
wire,  about  the  sixteenth  of  an  inch  from  the  point  of  the  blue 
cone.  In  the  pure  oxidation  flame,  a  clear  yellowish  glass  is 
formed  ;  but  as  soon  as  the  reduction  flame  reaches  it,  or  the 
point  of  the  blue  cone  touches  it,  the  color  of  the  bead  changes 
to  a  brown,  which,  finally,  after  a  little  longer  blowing,  becomes 
quite  dark,  and  loses  its  transparency.  The  cause  of  this  is, 
that  the  molybdenic  acid  is  very  easily  reduced  to  a  lower 
degree  of  oxidation,  or  to  the  oxide  of  molybdenum.  The 
flame  of  oxidation  will  again  convert  this  oxide  into  the  acid, 
and  this  conversion  is  a  good  test  of  the  progress  of  the  student 
in  the  use  of  the  blowpipe.  In  cases  where  we  have  to  sepa 
rate  a  more  oxidizable  substance  from  a  less  one,  we  use  with 
success  the  blue  cone,  particularly  if  we  wish  to  determine  whe 
ther  a  substance  has  the  .quality,  when  submitted  to  heat  in  the 
blue  cone,  of  coloring  the  external  flame. 

A  good  reduction  flame  can  be  obtained  by  the  use  of  a  small 
orifice  at  the  point  of  the  blowpipe.  In  order  to  produce  such 
a  flame,  hold  the  point  of  the  blowpipe  higher  above  the  wick, 
while  the  nozzle  must  not  enter  the  flame  so  far  as  in  the  pro 
duction  of  the  oxidation  flame.  The  point  of  the  blowpipe 
should  only  touch  the  flame,  while  the  current  of  air  blown  into 
it  must  be  stronger  than  into  the  oxidation  flame.  If  we  pro 
ject  a  stream,  in  the  manner  mentioned,  into  the  flame,  from 


20 


THE     BLOWPIPE. 


the  smaller  side  of  the  wick  to  the  middle,  we  shall  perceive  the 
flame  changed  to  a  long,  narrow,  luminous  cone,  a  b,  Fig.  4, 


the  end  a  of  which  is  enveloped  by  the  same  dimly  visible  blue- 
ish  colored  portion  of  the  flame  a,  c,  which  we  perceive  in  the 
original  flame,  with  its  point  at  c.  The  portion  close  above  the 
wick,  presenting  the  dull  appearance,  is  occasioned  by  the  rising 
gases  which  have  not  supplied  to  them  enough  oxygen  to  con 
sume  them  entirely.  The  hydrogen  is  consumed,  while  the 
carbon  is  separated  in  a  state  of  bright  ignition,  and  forms  the 
internal  flame. 

Directly  above  the  wick,  the  combustion  of  the  gases  is  least 
complete,  and  forms  there  likewise,  as  is  the  case  in  the  free 
flame,  a  dark  blue  nucleus  d. 

If  the  oxide  of  a  metal  is  brought  into  the  luminous  portion 
of  the  flame  produced  as  above,  so  that  the  flame  envelopes  the 
substance  perfectly,  the  access  of  air  is  prevented.  The  par 
tially  consumed  gases  have  now  a  strong  affinity  for  oxygen, 
under  the  influence  of  the  intense  heat  of  that  part  of  the  flame. 
The  substance  is  thus  deprived  of  a  part,  or  the  whole,  of  its 
oxygen,  and  becomes  reduced  according  to  the  strength  of  the  affin- 


I  T  S       U  S   K  .  21 

ity  which  the  substance  itself  has  for  oxygen.  If  the  reduction 
of  a  substance  is  undertaken  on  platinum,  by  fusion  with  a  flux, 
and  if  the  oxide  is  difficult  to  reduce,  the  reduction  will  be 
completely  effected  only  in  the  luminous  part  of  the  flame. 
But  if  a  substance  be  reduced  on  charcoal,  the  reduction  will 
take  place  in  the  blue  part  of  the  flame,  as  long  as  the  access  of 
air  is  cut  off ;  but  it  is  the  luminous  part  of  the  flame  which 
really  possesses  the  greatest  reducing  power. 

The  following  should  be  observed  in  order  to  procure  a  good 
reduction  flame  : 

The  wick  should  not  be  too  long,  that  it  may  make  a  smoke, 
nor  too  short,  otherwise  the  flame  will  be  too  small  to  produce 
a  heat  strong  enough  for  reduction. 

The  wick  must  be  free  from  all  loose  threads,  and  from  char 
coal. 

The  blast  should  be  continued  for  a  considerable  time  with 
out  intermission,  otherwise  reduction  cannot  be  effected. 

For  the  purpose  of  acquiring  practice,  the  student  may  fuse 
the  oxide  of  manganese  with  borax,  upon  a  platinum  wire,  in 
the  oxidation  flame,  when  a  violet-red  glass  will  be  obtained  ; 
or  if  too  much  of  the  oxide  be  used,  a  glass  of  a  dark  color  and 
opaque  will  be  obtained.  By  submitting  this  glass  to  the 
reduction  flame,  it  will  become  colorless  in  correspondence  to 
the  perfection  with  which  the  flame  is  produced.  Or  a  piece 
of  tin  may  be  fused  upon  charcoal,  and  kept  in  that  state  for  a 
considerable  time,  while  it  presents  the  appearance  of  a  bright 
metal  on  the  surface.  This  will  require  dexterity  in  the  opera 
tor  ;  for,  if  the  oxidation  flame  should  chance  to  touch  the 
bright  metal  only  for  a  moment,  it  is  coated  with  an  infusible 
oxide. 

COMBUSTION. — Any  flame  of  sufficient  size  can  be  used  for 
blowpipe  operations.  It  may  be  either  the  flame  of  a  candle 
of  tallow  or  wax,  or  the  flame  of  a  lamp.  The  flame  of  a  wax 
candle,  or  of  an  oil  lamp  is  most  generally  used.  Sometimes  a 
lamp  is  used  filled  with  a  solution  of  spirits  of  turpentine  in 
strong  alcohol.  If  a  candle  is  used,  it  is  well  to  cut  the  wick 


22 


THE     BLOWPIPE. 


off  short,  and  to  bend  the  wick  a  little  toward  the  substance 
experimented  upon.  But  candles  are  not  the  best  for  blowpipe 
operations,  as  the  radiant  heat,  reflecting  from  the  substance 
upon  the  wax  or  tallow,  will  cause  it  to  melt  and  run  down  the 
side  of  the  candle  ;  while  again,  candles  do  not  give  heat 
enough.  The  lamp  is  much  the  most  desirable.  The  subjoined 
figure,  from  Berzelius,  is  perhaps  the  best  form  of  lamp. 


It  is 


made  of  japanned  tin-plate,  about  four  inches  in  length,  and  has 


ITS     USE. 


23 


the  form  and  arrangement  represented  in  Fig.  5.  K  is  the  lamp, 
fastened  on  the  stand,  S,  by  a  screw,  C,  and  is  movable  upwards 
or  downwards,  as  represented  in  the  figure.  The  posterior  end  of 
the  lamp  may  be  about  one  inch  square,  and  at  its  anterior  end,  E, 
about  three-quarters  of  an  inch  square.  The  under  side  of  this  box 
may  be  round,  as  seen  in  the  figure.  The  oil  is  poured  into  the 
orifice,  A,  which  has  a  cap  screwed  over  it.  C'  is  a  wick- 
holder  for  a  flat  lamp-wick,  a  is  a  socket  containing  the  wick, 
which,  when  not  in  use,  is  secured  from  dirt  by  the  cap.  The 
figures  B  and  a'  give  the  forms  of  the  cap  and  socket.  The 
best  combustible  for  this  lamp  is  the  refined  rape-seed  oil,  or 
pure  sweet  oil.  When  this  lamp  is  in  use,  there  must  be  no 
loose  threads,  or  no  charcoal  on  the  wick,  or  these  will  produce 
a  smoky  flame.  The  wick,  likewise,  should  not  be  pulled  up 
too  high,  as  the  same  smoky  flame  would  be  produced. 

THE  SPIRIT-LAMP. — This  is  a  short,  strong  glass  lamp,  with 
a  cap,  B,  Fig.  6,  fitted  to  it  by  grinding,  to  prevent  the  cva- 


Fig.  G. 


poration  of  the  alcohol.     The  neck  a  contains  a  tube  C,  made 
of  silver,  or  of  tin  plate,  and  which  contains  the  wick.     Brass 


24:  T  H  E       B  L  O  W  P  I  P  K  . 

would  not  answer  so  well  for  this  tube,  as  the  spirits  would 
oxidize  it,  and  thus  impart  color  to  the  flame.  The  wickholder 
must  cover  the  edge  of  the  neck,  but  not  fit  tight  within  the 
tube,  otherwise,  by  its  expansion,  it  will  break  the  glass.  It 
is  not  necessary  that  alcohol,  very  highly  rectified,  should  be 
burnt  in.  this  lamp,  although  if  too  much  diluted  with  water, 
enough  heat  will  not  be  given  out.  Alcohol  of  specific  gravity 
0.84  to  0.86  is  the  best. 

This  lamp  is  generally  resorted  to  by  blowpipe  analysts,  for 
the  purpose  of  experiments  in  glass  apparatus,  as  the  oily  com 
bustibles  will  coat  the  glass  with  soot.  Some  substances,  when 
exposed  to  the  dark  part  of  the  flame,,  become  reduced  and,  in 
statu  nascendi,  evaporated  ;  but  by  passing  through  the  exter 
nal  part  of  the  flame,  they  became  oxidized  again,  and  impart 
a  color  to  the  flame.  The  spirit  flame  is  the  most  efficient  one 
for  the  examination  of  substances  the  nature  of  which  we  wish 
to  ascertain  through  color  imparted  to  the  flame,  as  that  of 
the  spirit-lamp  being  colorless,  is,  consequently,  most  easily 
and  thoroughly  recognized  by  the  slightest  tinge  imparted  to  it. 
It  is  necessary  that  in  operating  with  such  minute  quanti 
ties  of  substances  as  are  used  in  blowpipe  analysis,  that  they 
should  have  some  appropriate  support.  In  order  that  no  false 
results  may  ensue,  it  is  necessary  that  the  supports  should  be  of 
such  a  nature  that  they  will  not  form  a  chemical  combination 
with  the  substance  while  it  is  exposed  to  fusion  or  ignition. 
Appropriate  supports  for  the  different  blowpipe  experiments  are 
charcoal,  platinum  instruments,  and  glass  tubes. 

(a.)    Charcoal. — The  value  of  charcoal  as  a  support  may  be 
stated  as  follows  : 

1.  The  charcoal  is  infusible,  and  being  a  poor  conductor  of 
beat,  a  substance  can  be  exposed  to  a  higher  degree  of  heat 
upon  it  than  upon  any  other  substance. 

2.  It  is  very  porous,  and  therefore  allows  easily  fusible  sub 
stances  (such  as  alkalies  and  fluxes)  to  pass  into  it,  while  other 
substances  less  fusible,  such  as  metals,  to  remain  unabsorbed. 

3.  It  has  likewise  a  great  reducing  power. 


I  T  S      U  8  E.  25 

The  best  kind  of  charcoal  is  that  of  pinewood,  linden,  ivillow, 
or  alderwood,  or  any  other  soft  wood.  Coal  from  the  firwood 
sparkles  too  freely,  while  that  of  the  hard  woods  contains  too 
much  iron  in  its  ashes.  Smooth  pieces,  free  from  bark  and 
knots,  should  be  selected.  It  should  be  thoroughly  burnt,  and 
the  annual  rings  or  growths  should  be  as  close  together  as 
possible. 

If  the  charcoal  is  in  masses,  it  should  be  sawed  into  pieces 
about  six  inches  in  length  by  about  two  inches  broad,  but  so 
that  the  year-growths  run  perpendicular  to  the  broadest  side, 
as  the  other  sides,  by  their  unequal  structure,  burn  unevenly. 

That  the  substance  under  examination  may  not  be  carried 
off  by  the  blast,  small  conical  concavities  should  be  cut  in  the 
broad  side  of  the  charcoal,  between  the  year-growths,  with  a 
conical  tube  of  tin  plate  about  two  or  three  inches  long,  and 
one  quarter  of  an  inch  at  one  end,  and  half  an  inch  at  the 
other.  These  edges  are  made  sharp  with  a  file.  The  widest 
end  of  this  charcoal  borer  is  used  for  the  purpose  of  making 
cavities  for  cupellation. 

In  places  where  the  proper  kind  of  charcoal  is  difficult  to 
procure,  it  is  economical  to  cut  common  charcoal  into  pieces 
about  an  inch  broad,  and  the  third  of  an  inch  thick.  In  each 
of  these  little  pieces  small  cavities  should  be  cut  with  the  small 
end  of  the  borer.  When  these  pieces  of  charcoal  are  required 
for  use,  they  must  be  fastened  to  a  narrow  slip  of  tin  plate, 
one  end  of  which  is  bent  into  the  form  of  a  hook,  under  which 
the  plate  of  charcoal  is  pushed. 

In  general,  we  use  the  charcoal  support  where  we  wish  to 
reduce  metallic  oxides,  to  prevent  oxidation,  or  to  test  the 
fusibility  of  a  substance.  There  is  another  point  to  which  we 
would  direct  the  student.  Those  metals  which  are  volatile  in 
the  reduction  flame,  appear  as  oxides  in  the  oxidation  flame. 
These  oxides  make  sublimates  upon  the  charcoal  close  in  the 
vicinity  of  the  substance,  or  where  it  rested,  and  by  their  pecu 
liar  color  indicate  pretty  correctly  the  species  of  minerals  ex 
perimented  upon. 


26  THE    BLOWPIPE. 

(Z>.)  Platinum  Supports. — The  metal  platinum  is  infusible  in 
the  blowpipe  flame,  and  is  such  a  poor  conductor  of  heat  that 
a  strip  of  it  may  be  held  close  to  that  portion  of  it  which  is 
red  hot  without  the  least  inconvenience  to  the  fingers.     It  is 
necessary  that  the  student  should  be  cognizant  of  those  sub 
stances  which  would  not  be  appropriate  to  experiment  upon 
if  placed  on  platinum.     Metals  should  not  be  treated  upon 
platinum   apparatus,   nor  should  the   easily  reducible   oxides, 
sulphides,  nor  chlorides,  as  these  substances  will  combine  with 
the  platinum,  and  thus  render  it  unfit  for  further  use  in  analysis. 
(c.)  Platinum  Wire. — As  the  color  of  the  flame  cannot  be 
well  discerned  when  the  substance  is  supported  upon  charcoal, 
in  consequence  of  the  latter  furnishing  false  colors,  by  its  own 
reflection,  to  the  substances  under  examination,  we  use  plati 
num  wire  for  that  purpose,  when  we  wish  to  examine  those 
substances  which  give  indications  by  the  peculiar  color  which 
they  impart  to  fluxes.      The  wire  should  be  about  as  thick 
as    No.    16     or    18    wire,    or    about    0.4    millimetre,    and 
cut  into  pieces  about  from  two  and  a  half  to  three  inches 
in    length.     The    end    of    each  piece  is  crooked.     In    order 
that    these    pieces  should   remain    clear    of  dirt,    and   ready 
for  use,  they  should  be  kept  -in  a  glass  of  water.     To  use 
them,  we  dip  the  wetted  hooked  end  into  the  powdered  flux 
(borax  or  microcosmic  salt)  some  of  which  will  adhere,  when 
we  fuse  it  in  the  flame  of  the  blowpipe  to  a  bead.     This  bead 
hanging  in  the  hook,  must  be  clear  and   colorless.     Should 
there  not  adhere  a  sufficient  quantity  of  the  flux  in  the  first 
trial  to  form  a  bead  sufficiently  large,  the  hook  must  be  dipped 
a  second  time  in  the  flux  and  again  submitted  to  the  blowpipe 
flame.     To  fix  the  substance  to  be  examined  to  the  bead,  it  is 
necessary,  while  the  latter  is  hot,  to  dip  it  in  the  powdered 
substance.     If  the  hook  is  cold,  we  moisten  the  powder  a  little, 
and  then  dip  the  hook  into  it,  and  then  expose  it  to  the  oxida 
tion  flame,  by  keeping  it  exposed  to  a  regular  blast  until  the 
substance  and  the  flux  are  fused  together,  and  no  further  alter 
ation  is  produced  by  the  flame. 


I  T  S     U  S  E  .  27 

The  platinum  wire  can  be  used  except  where  reduction  to 
the  metallic  state  is  required.  Every  reduction  and  oxidation 
experiment,  if  the  results  are  to  be  known  by  the  color  of  the 
fluxes,  should  be  effected  upon  platinum  wire.  At  the  termina 
tion  of  the  experiment  or  investigation,  if  it  be  one,  to  clean 
the  wire,  place  it  in  water,  which  will  dissolve  the  bead. 

(d.)  Platinum  Foil. — For  the  heating  or  fusing  of  a  substance, 
whereby  its  reduction  would  be  avoided,  we  use  platinum  foil 
as  a  support.  This  foil  should  be  of  the  thickness  of  good 
writing  paper,  and  from  two  and  a  half  to  three  inches  long, 
by  about  half  an  inch  broad,  and  as  even  and  smooth  as  possi 
ble.  If  it  should  become  injured  by  long  use,  cut  the  injured 
end  off,  and  if  it  should  prove  too  short  to  be  held  with  the 
fingers,  a  pair  of  forceps  may  be  used  to  grasp  it,  or  it  may  be 
placed  on  a  piece  of  charcoal 

(e.)  Platinum  Spoon. — When  we  require  to  fuse  substances 
with  the  acid  sulphate  of  potash,  or  to  oxidize  them  by 
detonation  with  nitrate  of  potash,  whereby  we  wish  to  preserve 
the  oxide  produced,  we  generally  use  a  little  spoon  of  plati 
num,  about  from  nine  to  fifteen  millimetres  *  in  diameter,  and 
shaped  as  represented  in  Fig.  1.  The  handle  of  this  spoon  is 


Fig.  7. 

likewise  of  platinum,  and  should  fit  into  a  piece  of  cork,  or  be 
held  with  the  forceps. 

(/.)  Platinum  Forceps  or  Tongs. — We  frequently  are  neces 
sitated  to  examine  small  splinters  of  metals  or  minerals 
directly  in  the  blowpipe  flame.  These  pieces  of  metallic  sub 
stances  are  held  with  the  forceps  or  tongs  represented  as  in 

*  The  French  millimetre  is  about  the  twenty -fifth  part  of  an  English  inch. 


28  THE     BLOW  PIPE. 

Fig.  8,  where  a  c  is  formed  of  steel,  and  a  a  are  platinum 


Fig.  8. 

bars  inserted  between  the  steel  plates.  At  b  b  are  knobs 
which  by  pressure  so  separate  the  platinum  bars  a  a,  that  any 
small  substance  can  be  inserted  between  them. 

(g.)  Iron  Spoons. — For  a  preliminary  examination  iron  spoons 
are  desirable.  They  may  be  made  of  sheet  iron,  about 
one-third  of  an  inch  in  diameter,  and  are  very  useful  in  many 
examinations  where  the  use  of  platinum  would  not  be 
desirable. 

(h.)  Glass  Tubes. — For  the  separation  and  recognition  of 
volatile  substances  before  the  blowpipe  flame,  we  use  glass 
tubes.  These  should  be  about  one-eighth  of  an  inch  in  diame 
ter,  and  cut  into  pieces  about  five  or  six  inches  in  length. 
These  tubes  should  have  both  ends  open. 

Tubes  are  of  great  value  in  the  examination  of  volatile  sub 
stances  which  require  oxidizing  or  roasting,  and  heating  with 
free  access  of  air.  Also  to  ascertain  whether  a  substance 
under  examination  will  sublimate  volatile  matter  of  a  certain 
appearance.  Such  substances  are  selenium,  sulphur,  arsenic, 
antimony,  and  tellurium.  These  substances  condense  on  a  cool 
part  of  the  tube,  and  they  present  characteristic  appearances,  or 
they  may  be  recognized  by  their  peculiar  smell.  These  tubes 
must  be  made  of  the  best  kind  of  glass,  white  and  difficult  of 
fusion,  and  entirely  free  from  lead.  The  substance  to  be 
examined  must  be  put  in  the  tube  near  one  end,  and  exposed 
to  the  flame  of  the  blowpipe.  The  end  containing  the  sub 
stance  must  be  held  lower  than  the  other  end,  and  must  be 
moved  a  little  over  the  spirit-lamp  before  a  draught  of  air  is 
produced  through  the  tube.  It  is  a  good  plan  to  have  a  number 


I  T  S       II  8  1C  .  29 

of  these  tubes  on  hand.  After  having  used  a  tube  we  cut  off 
that  end  of  it  which  contained  the  substance,  with  a  file,  and 
clean  it  from  the  sublimate,  either  by  heating  it  over  the 
spirit-lamp,  or  with  a  piece  of  paper  wound  around  a  wire.  It 
sometimes  happens  that  the  substance  falls  out  of  the  tube 


Fig.  9. 


30 


THE    BLOWPIPE. 


before  it  becomes  sufficiently  melted  to  adhere  to  the  glass. 
To  obviate  this,  we  bend  the  tube  not  far  from  the  end,  at  an 
obtuse  angle,  and  place  the  substance  in  the  angle,  whereby 
the  tube  may  be  lowered  as  much  as  necessary.  Fig.  9  will 
give  the  student  a  comprehension  of  the  processes  described, 
and  of  the  manner  of  bending  the  tubes. 

(i.)  Glass  Tubes  closed  at  one  End. — If  we  wish  to  expose 
volatile  substances  to  heat,  with  the  exclusion  of  air  as  much 
as  possible,  or  to  ascertain  the  contents  of  water,  or  other 
volatile  fluids,  or  for  the  purpose  of  heating  substances  which 
will  decrepitate,  we  use  glass  tubes  closed  at  one  end.  These 
tubes  must  be  about  one-eighth  of  an  inch  wide,  and  from 
two  to  three  inches  in  length.  They  should  be  made  of  white 
glass,  difficult  of  fusion,  and  free  from  lead.  They  should  be 
closed  at  one  end,  as  figured  in  the  margin,  Fig.  10. 


Fig.  10. 


When  a  substance  is  to  be  examined  for  the  purpose  of 


I  T  S       U  8  E  .  31 

ascertaining  whether  it  contains  combustible  matter,  as  sulphur 
or  arsenic,  and  where  we  wish  to  avoid  oxidation,  we  use  these 
tubes  without  extending  the  closed  end,  in  order  that  there 
may  be  as  little  air  admitted  as  possible,  as  is  represented  in 
tube  B.  But  when  a  substance  to  be  examined  is  to  be  tested 
for  water,  or  other  incombustible  volatile  matters,  we  employ 
tubes  with  little  bulbs  blown  at  one  end,  such  as  represented  at 
tube  A.  Here  there  is  room  for  a  circulation  of  air  at  the  bot 
tom  of  the  tube,  by  which  the  volatile  matter  rises  more  easily. 
In  some  cases,  it  is  necessary  to  draw  the  closed  end  out  to  a 
fine  point,  as  in  the  tubes  C  and  D.  Either  one  or  the  other  of 
these  tubes  is  employed,  depending  upon  the  nature  of  the  sub 
stance  used.  The  sublimates  condense  at  the  upper  part  of  the 
tube  a,  and  can  be  there  examined  and  recognized.  These  tubes, 
before  being  used,  must  be  thoroughly  dried  and  cleaned.  In 
experimenting  with  them,  they  should  not  be  exposed  at  once 
to  the  hottest  part  of  the  flame,  but  should  be  submitted  to  the 
heat  gradually.  If  the  substance  is  of  such  a  nature  that  it 
will  sublime  at  a  low  heat,  the  tube  should  be  held  more  hori 
zontal,  while  a  higher  heat  is  attained  by  bringing  the  tube  to 
a  more  vertical  position. 


VARIOUS  APPARATUS  NECESSARY. 

Edulcorator  or  Washing  Bottle. — Take  a  glass  bottle  of  the 
capacity  of  about  twelve  ounces,  and  close  the  mouth  of  it  very 
tight  with  a  cork,  through  which  a  short  glass*  tube  is  fitted 
airtight.  The  external  end  of  this  tube  is  drawn  out  to  a 
point,  with  a  very  fine  orifice.  The  bottle  should  be  filled 
about  half  full  of  water.  By  blowing  air  into  the  bottle 
through  the  tube,  and  then  turning  it  downwards,  the  com 
pressed  air  will  expel  a  fine  stream  of  water  through  the  fine 
orifice  with  considerable  force.  We  use  this  washing  bottle, 
Fig.  11,  for  the  purpose  of  rinsing  the  small  particles  of  coal 
from  the  reduced  metals. 


32  THEBLOWPIP 


Fig.  11. 

Agate  Mortar  and  Pestle. — This  mortar  is  used  for  the  purpose 
of  pulverizing  hard  substances,  and  for  mixing  fluxes.  As  this 
mortar  will  not  yield  to  abrasion,  there  is  no  danger  of  any 
foreign  matter  becoming  mixed  with  the  substance  pulverized 
in  it.  It  should  be  cleaned  after  use  with  pumice  stone.  Steel 
mortars  are  very  useful  for  the  pulverization  of  hard  bodies  ; 
but  for  all  those  substances  which  require  great  care  in  their 
analysis,  and  which  can  be  obtained  in  very  minute  quantity, 
the  agate  mortar  alone  should  be  used. 

A  hammer  made  of  steel  is  necessary.  This  should  have  the 
edge  square. 

A  small  anvil,  polished  on  the  surface,  is  also  required.  It  is 
frequently  used  to  test  the  malleability  of  metals. 

A  knife,  for  the  purpose  of  ascertaining  the  hardness  of  mine 
rals. 

The  student  should  also  be  provided  with  several  three-edged 
files,  and  likewise  with  some  flat  ones. 

A  microscope,  an  instrument  with  two  lenses,  or  with  such  a 
combination  of  lenses,  that  they  may  be  used  double  or  single, 


ITS     USE. 


S3 


is  frequently  necessary  for  the  examination  of  blowpipe  experi 
ments,  or  the  reaction  of  the  fluxes.  Common  lenses,  howso 
ever  cheap  they  may  be,  are  certainly  not  recommended.  A 
microscope  with  achromatic  lenses  can  now  be  purchased  so 
cheap  that  there  is  no  longer  any  necessity  of  procuring  one 
with  the  common  lens.  Besides,  there  is  no  reliability  whatever 
to  be  placed  in  the  revelations  of  the  common  lens  ;  while  on 
the  contrary,  the  deceptive  appearances  which  minute  objects 
assume  beneath  such  lenses  are  more  injurious  than  otherwise. 
A  small  cheap  set  of  magnifying  glasses  are  all  that  is  required 
for  the  purpose  of  blowpipe  analysis,  Fig.  12. 


Fig.  12. 

A  small  magnet  should  be  kept  on  hand,  for  the  purpose  of 
testing  reduced  metals. 

Nippers,  for  the  purpose  of  breaking  off  pieces  of  minerals 
for  analysis,  without  injuring  the  entire  piece,  are  indispensable, 
Fig  13. 


Fig.  18. 

A  pair  of  scissors  is  required  to  trim  the  wick  of  the  lamp? 
and  for  the  trimming  of  the  edge  of  platinum  foil. 

2* 


34:  THE     BLOW  PIPE. 

A  small  spatula  should  be  kept  for  the  purpose  of  mixing 
substances  with  fluxes. 


THE   REAGENTS. 

Those  substances  which  possess  the  property  of  acting  upon 
other  substances,  in  such  a  characteristic  manner  that  they  can 
be  recognized,  either  by  their  color,  or  by  their  effervescence, 
or  by  the  peculiar  precipitation  produced,  are  termed  reagents. 
The  phenomena  thus  produced  is  termed  reaction.  We  use 
those  reagents,  or  tests,  for  the  purpose  of  ascertaining  the 
presence  or  the  absence  of  certain  substances,  through  the 
peculiar  phenomena  produced  when  brought  in  contact  with 
them. 

The  number  of  reagents  employed  in  blowpipe  analysis  is  not 
great,  and  therefore  we  shall  here  give  a  brief  description  of  their 
preparation  and  use.  It  is  indispensably  necessary  that  they 
should  be  chemically  pure,  as  every  admixture  of  a  foreign  sub 
stance  would  only  produce  a  false  result.  Some  of  them  have 
a  strong  affinity  for  water,  or  are  deliquescent,  and  consequently 
absorb  it  greedily  from  the  air.  These  must  be  kept  in  glass 
bottles,  with  glass  stoppers,  fitted  air-tight  by  grinding. 

A.    REAGENTS    OF    GENERAL   USE. 

1.  Carbonate  of  Soda. — (NaO,  CO2)  Wash  the  bicarbonate 
of  soda  (NaO,  2C02)  upon  a  filter,  with  cold  water,  until  the 
filtrate  ceases  to  give,  after  neutralization  with  diluted  nitric 
acid  (NO5),  a  precipitate  with  nitrate  of  baryta,  (BaO,  NO6), 
or  nitrate  of  silver,  (AgO,  NO5).  That  left  upon  the  filter 
we  make  red  hot  in  a  platinum,  silver,  or  porcelain  dish.  One 
atom  of  carbonic  acid  is  expelled,  and  the  residue  is  carbonate 
of  soda. 

A  solution  of  soda  must  not  be  changed  by  the  addition  of 
sulphide  of  ammonium.  And  when  neutralized  with  hydro 
chloric  acid,  and  evaporated  to  dryness,  and  again  dissolved 
in  water,  there  must  be  no  residue  left. 


I  T  8       IT  S  E  .  35 

Carbonate  of  soda  is  an  excellent  agent  in  reduction,  in 
consequence  of  its  easy  fusibility,  whereby  it  causes  the  close 
contact  of  the  oxides  with  the  charcoal  support,  so  that  the 
blowpipe  flame  can  reach  every  part  of  the  substance  under 
examination. 

For  the  decomposition  and  determination  of  insoluble  sub 
stances,  particularly  the  silicates,  carbonate  of  soda  is  indis 
pensable.  But  for  the  latter  purpose,  we  use  with  advantage 
a  mixture  of  ten  parts  of  soda  and  thirteen  parts  of  dry  car 
bonate  of  potash,  which  mixture  fuses  more  easily  than  the 
carbonate  of  soda  alone. 

2.  Hydrate  of  Baryta  (BaO,  HO). — This  salt  is  used  some 
times  for  the  detection  of  alkalies  in  silicates.     Mix  one  part 
of  the  substance  with  about  four  parts  of  the  hydrate  of  baryta, 
and  expose  it  to  the  blowpipe  flame.     The  hydrate  of  baryta 
combines  with  the  silicic  acid,  and  forms  the  super-basic  silicate 
of  baryta,  while  the  oxides  become  free.     The  fused  mass  must 
be  dissolved  in  hydrochloric  acid,  which  converts  the  oxides 
into  chlorides.     Evaporate  to  dryness,  and  dissolve  the  residue 
in  water.     The  silicic  acid  remains  insoluble. 

The  hydrate  of  baryta  is  prepared  by  mixing  six  parts  of 
finely  powdered  heavy-spar  (BaO,  S03)  with  one  part  of  char 
coal  and  one  and  a  half  parts  of  wheat  flour,  and  exposing 
this  mixture  in  a  Hessian  crucible  with  a  cover  to  a  strong  and 
continuous  red  heat.  The  coaled  chocolate-brown  mass  must 
be  boiled  with  twenty  parts  of  water,  and,  while  boiling,  there 
must  be  added  the  oxide  of  copper  in  sufficient  quantity,  or 
until  the  liquid  will  not  impart  a  black  color  to  a  solution  of 
acetate  of  lead  (PbO,  A).  The  liquid  must  be  filtered  while 
hot,  and  as  it  cools  the  hydrate  of  baryta  appears  in  crystals. 
These  crystals  must  be  washed  with  a  little  cold  water,  and 
then  heated  at  a  low  temperature  in  a  porcelain  dish  until  the 
crystal  water  is  expelled.  The  hydrate  of  baryta  melts  by  a 
low  red  heat  without  losing  its  water  of  hydration. 

3.  Bisulphate  of  Potassa  (KO,  2S03). — At  a  red  heat  the 
half  of  the  sulphuric  acid  of  this  salt  becomes  free,  and  thus 


36  THE    BLOWPIPE. 

separates  and  expels  volatile  substances,  by  which  we  can 
recognize  lithium,  boracic  acid,  nitric  acid,  fluoric  acid,  bromine, 
iodine,  chlorine  ;  or  it  decomposes  and  reveals  some  other 
compounds,  as,  for  instance,  the  salts  of  the  titanic,  tantalic 
and  tungstic  acids.  The  bisulphate  of  potash  is  also  used  for 
the  purpose  of  converting  a  substance  into  sulphate,  or  to  free 
it  at  once  from  certain  constituents.  These  sulphates  are  dis 
solved  in  water,  by  which  we  are  enabled  to  effect  the  sepa 
ration  of  its  various  constituents. 

PREPARATION. — Two  parts  of  coarsely  powdered  sulphate  of 
potash  are  placed  in  a  porcelain  crucible,  and  one  part  of  pure 
sulphuric  acid  is  poured  over  it.  Expose  this  to  heat  over  the 
spirit-lamp,  until  the  whole  becomes  a  clear  liquid.  The  cooled 
mass  must  be  of  a  pure  white  color,  and  may  be  got  out  of  the 
crucible  by  inverting  it.  It  must  be  kept  in  a  fine  powder. 

4.  Oxalate  of  Potassa  (KO ,  0). — Dissolve  bioxalate  of  pot 
ash  in  water,  and  neutralize  with  carbonate  of  potash.     Evapo 
rate  the  solution  at  a  low  heat  to  dryness,  stirring  constantly 
towards  the  close  of  the  operation.     The  dry  residue  is  to  be 
kept  in  the  form  of  a  powder. 

The  oxalate  of  potash,  at  a  low  red  heat,  eliminates  a  consid 
erable  quantity  of  carbonic  oxide,  which,  having  a  strong 
affinity  for  oxygen,  with  which  it  forms  carbonic  acid,  it  is 
therefore  a  powerful  agent  of  reduction.  It  is  in  many  cases 
preferable  to  carbonate  of  soda. 

5.  Cyanide  of  Potassium  (Cy,  K). — In  the  dry  method  of 
analysis,  this  salt  is  one  of  the  most  efficient  agents  for  the 
reduction  of  metallic  oxides.     It  separates  not  only  the  metals 
from  their  oxygen  compounds,  but  likewise  from  their  sulphur 
compounds,  while  it  is  converted  through  the  action  of  the 
oxygen  into  carbonate  of  potash,  or,  in  the  latter  case,  combines 
with  the  sulphur  and  forms  the  sulphureted  cyanide  of  potassium. 
This  separation  is  facilitated  by  its   easy  fusibility.     But  in 
many  cases  it  melts  too  freely,  and  therefore  it  is  better  to  mix 
it,  for  blowpipe  analysis,  with  an  equal  quantity  of  soda.     This 
mixture  has  great  powers  of  reduction,   and  it  is   easily  ab- 


I  T  S       U  S  E  .  37 

sorbed  by  the  charcoal,  while  the  globules  of  reduced  metal 
are  visible  in  the  greatest  purity. 

PREPARATION. — Deprive  the  ferrocyanide  of  potassium  (2KCy 
+  FeCy)  of  its  water  by  heating  it  over  the  spirit-lamp 
in  a  porcelain  dish.  Mix  eight  parts  of  this  anhydrous  salt 
with  three  parts  of  dry  carbonate  of  potash,  and  fuse  the 
mixture  by  a  low  red  heat  in  a  Hessian,  or  still  better,  in  an 
iron  crucible  with  a  cover,  until  the  mass  flows  quiet  and  clear, 
and  a  sample  taken  up  with  an  iron  spatula  appears  perfectly 
white.  Pour  the  clear  mass  out  into  a  china  or  porcelain  dish 
or  an  iron  plate,  but  with  caution  that  the  fine  iron  par 
ticles  which  have  settled  to  the  bottom,  do  not  mix  with  it. 
The  white  fused  mass  must  be  powdered,  and  kept  from 
the  air.  The  cyanide  of  potassium  thus  prepared,  contains 
some  of  the  cyanate  of  potassa,  but  the  admixture  does  not 
deteriorate  it  for  blowpipe  use.  It  must  be  perfectly  white, 
free  from  iron,  charcoal,  and  sulphide  of  potassium.  The  solu 
tion  of  it  in  water  must  give  a  white  precipitate  with  a  solution 
of  lead,  and  when  neutralized  with  hydrochloric  acid,  and 
evaporated  to  dryness,  it  must  not  give  an  insoluble  residue  by 
dissolving  it  again  in  water. 

6.  Nitrate  of  Potassa,  Saltpetre  (KO,  NO6).— Saturate  boil 
ing  water  with  commercial  saltpetre,  filter  while  hot  in  a 
beaker  glass,  which  is  to  be  placed  in  cold  water,  and  stir 
while  the  solution  is  cooling.  The  greater  part  of  the  salt 
petre  will  crystallize  in  very  fine  crystals.  Place  these  crystals 
upon  a  filter,  and  wash  them  with  a  little  cold  water,  until  a 
solution  of  nitrate  of  silver  ceases  to  exhibit  any  reaction  upon 
the  filtrate.  These  crystals  must  be  dried  and  powdered. 

Saltpetre,  when  heated  with  substances  easy  of  oxidation, 
yields  its  oxygen  quite  readily,  and  is,  therefore,  a  powerful 
means  of  oxidation.  In  blowpipe  analysis,  we  use  it  particu 
larly  to  convert  sulphides  (as  those  of  arsenic,  antimony,  &c.) 
into  oxides  and  acids.  We  furthermore  use  saltpetre  for  the 
purpose  of  producing  a  complete  oxidation  of  small  quantities 
of  metallic  oxides,  which  oxidize  with  difficulty  in  the  oxidation 


38  THE    BLOWPIPE. 

flame,  so  that  the  color  of  the  bead,  in  its  highest  state  of  oxi 
dation,  shall  be  visible,  as  for  instance,  manganese  dissolved  in 
the  microcosmic  salt. 

1.  Biborate  of  soda,  borax — (NaO  +  2B03). — Commercial 
borax  is  seldom  pure  enough  for  a  reagent.  A  solution  of 
borax  must  not  give  a  precipitate  with  carbonate  of  potassa  ; 
or,  after  the  addition  of  dilute  nitric  acid,  it  must  remain  clear 
upon  the  addition  of  nitrate  of  silver,  or  nitrate  of  baryta.  Or 
a  small  piece  of  the  dry  salt,  fused  upon  a  platinum  wire,  must 
give  a  clear  and  uncolored  glass,  as  well  in  the  oxidation  flame 
as  in  the  reduction  flame.  If  these  tests  indicate  a  foreign 
admixture,  the  borax  must  be  purified  by  re-crystallization. 
These  crystals  are  washed  upon  a  filter,  dried,  and  heated,  to 
expel  the  crystal  water,  or  until  the  mass  ceases  to  swell  up, 
and  it  is  reduced  to  powder. 

Boracic  acid  is  incombustible,  and  has  a  strong  affinity  for 
oxides  when  fused  with  them ;  therefore,  it  not  only  directly 
combines  with  oxides,  but  it  expels,  by  fusion,  all  other  volatile 
acids  from  their  salts.  Furthermore,  boracic  acid  promotes  the 
oxidation  of  metals  and  sulphur,  and  induces  haloid  compounds, 
in  the  oxidation  flame,  to  combine  with  the  rising  oxides. 
Borates  thus  made,  melt  generally  by  themselves  ;  but  admixed 
with  borate  of  soda,  they  fnse  much  more  readily,  give  a  clear 
bead.  Borax  acts  either  as  a  flux,  or  through  the  formation 
of  double  salts. 

In  borax,  we  have  the  action  of  free  boracic  acid,  as  well  as 
borate  of  soda,  and  for  that  reason  it  is  an  excellent  reagent  for 
blowpipe  analysis. 

All  experiments  in  which  borax  is  employed  should  be  effected 
upon  platinum  wire.  The  hook  of  the  wire  should  be  heated 
red  hot,  and  then  dipped  into  the  powdered  borax.  This  should 
be  exposed  to  the  oxidation  flame,  when  it  will  be  fused  to  a 
bead,  which  adheres  to  the  hook.  This  should  be  then  dipped 
into  the  powdered  substance,  which  will  adhere  to  it  if  it  is 
hot ;  but  if  the  bead  is  cool,  it  must  be  previously  moistened. 
Expose  this  bead  to  the  oxidation  flame  until  it  ceases  to 


I  T  S       U  S  E  .  39 

change,  then  allow  it  to  cool,  when  it  should  be  exposed  to  the 
reduction  flame.  Look  for  the  following  in  the  oxidation  flame  : 

(1.)  Whether  the  heated  substance  is  fused  to  a  clear  bead  or 
not,  and  whether  the  bead  remains  transparent  after  cooling. 
The  beads  of  some  substances,  for  instance  those  of  the  alkaline 
earths,  are  clear  while  hot  ;  but  upon  cooling,  are  milk-white 
and  enamelled.  Some  substances  give  a  clear  bead  when  heated 
and  when  cold,  but  appear  enamelled  when  heated  intermittingly 
or  with  a  flame  which  changes  often  from  oxidation  to  reduction, 
or  with  an  unsteady  flame  produced  by  too  strong  a  blast.  The 
reason  is  an  incomplete  fusion,  while  from  the  basic  borate  com 
pound  a  part  of  the  base  is  separated.  As  the  boracic  acid  is 
capable  of  dissolving  more  in  the  heat,  a  bead  will  be  clear  while 
hot,  enamelled  when  cold,  as  a  part  in  the  latter  instance  will 
become  separated. 

(2.)  Whether  the  substance  dissolves  easily  or  not,  and 
whether  it  intumesces  from  arising  gases. 

(3.)  Whether  the  bead,  when  exposed  to  the  oxidation  flame, 
exhibits  any  color,  and  whether  the  color  remains  after  the 
bead  shall  have  cooled,  or  whether  the  color  fades. 

(4.)  Whether  the  bead  exhibits  any  other  reaction  in  the 
reduction  flame. 

The  bead  should  not  be  overcharged  with  the  substance  under 
examination,  or  it  will  become  colored  so  deeply  as  not  to 
present  any  transparency,  or  the  color  light  enough  to  discern 
its  hue. 

8.  Microcosmic  Salt — Phosphate  of  Soda  and  Ammonia — 
(NaO,  NH*0  +  P05).— Dissolve  six  parts  of  phosphate  of 
soda  (2NaO,  HO,  PO6),  and  one  part  of  pure  chloride  of 
Ammonium  (NH4C1.),  in  two  parts  of  boiling  water,  and  allow 
it  to  cool.  The  greatest  part  of  the  formed  double  salt  crys 
tallizes,  while  the  mother-liquid  contains  chloride  of  sodium, 
and  some  of  the  double  salt.  The  crystals  must  be  dissolved  in 
as  little  boiling  water  as  possible,  and  re-crystallized.  These 
crystals  must  be  dried  and  powdered. 

When  this  double  salt  is  heated,  the  water  and  the  ammonia, 


40  THE     BLOW  PIPE. 

escape,  while  the  incombustible  residue  has  a  composition  simi 
lar  to  borax,  viz.,  a  free  acid  and  an  easily  fusible  salt.  The 
effect  of  it  is,  therefore,  similar  to  the  borax.  The  free  phos 
phoric  acid  expels,  likewise,  most  other  acids  from  their  combi 
nations,  and  combines  with  metallic  oxides. 

For  supports,  the  platinum  wire  may  be  used,  but  the  hook 
must  be  smaller  than  when  borax  is  used,  or  the  bead  will  not 
adhere.  As  for  all  the  other  experiments  with  this  salt,  the 
microscosmic  salt  is  used  the  same  as  borax. 

9.  Nitrate  of  Cobalt. — (CoO,  NO5). — This  salt  can  be  pre 
pared  by  dissolving  pure  oxide  of  cobalt  in  diluted  nitric  acid, 
and  evaporating  to  dryness  with  a  low  heat.  The  dry  residue 
should  be  dissolved  in  ten  parts  of  water,  and  filtered.  The 
filtrate  is  now  ready  for  use,  and  should  be  kept  in  a  bottle 
with  a  glass  stopper.  If  the  pure  oxide  of  cobalt  cannot  be 
procured,  then  it  may  be  prepared  by  mixing  two  parts  of  finely 
powdered  glance  of  cobalt  with  four  parts  of  saltpetre,  and  one 
part  of  dry  carbonate  of  potassa  with  one  part  of  water  free 
from  carbonate  of  soda.  This  mixture  should  be  added  in  suc 
cessive  portions  into  a  red-hot  Hessian  crucible,  and  the  heat 
continued  until  the  mass  is  fused,  or  at  least  greatly  diminished 
in  volume.  The  cooled  mass  must  be  triturated  with  hot  water, 
a.nd  then  heated  with  hydrochloric  acid  until  it  is  dissolved  and 
forms  a  dark  green  solution,  which  generally  presents  a  gelati 
nous  appearance,  occasioned  by  separated  silica.  The  solution 
is  to  be  evaporated  to  dryness,  the  dry  residue  moistened  with 
hydrochloric  acid,  boiled  with  water,  filtered  and  neutralized 
while  hot  with  carbonate  of  ammonia,  until  it  ceases  to  give 
an  acid  reaction  with  test-paper.  This  must  now  be  filtered 
again,  and  carbonate  of  potassa  added  to  the  filtrate  as  long  as 
a  precipitate  is  produced.  This  precipitate  is  brought  upon  a  filter 
and  washed  thoroughly,  and  then  dissolved  in  diluted  nitric  acid. 
This  is  evaporated  to  dryness,  and  one  part  of  it  is  dissolved  in 
ten  parts  of  water  for  use. 

The  oxide  of  cobalt  combines,  with  strong  heat  in  the 
oxidation  flame,  with  various  earths  and  infusible  metallic 


I  T  8       U  8  E  .  41 

oxides,  and  thus  produces  peculiarly  colored  compounds,  and 
is  therefore  used  for  their  detection  ;  (alumina,  magnesia,  oxide 
of  zinc,  oxide  of  tin,  etc.)  Some  of  the  powdered  substance 
is  heated  upon  charcoal  in  the  flame  of  oxidation,  and  moist 
ened  with  a  drop  of  the  solution  of  the  nitrate  of  cobalt,  when 
the  oxidation  flame  is  thrown  upon  it.  Alumina  gives  a  pure 
blue  color,  the  oxide  of  zinc  a  bright  green,  magnesia  a  light 
red,  and  the  oxide  of  tin  a  bluish-green  color  ;  but  the  latter 
is  only  distinctly  visible  after  cooling. 

The  dropping  bottle,  is  the  most  useful  apparatus  for 
the  purpose  of  getting  small  quantities  of  fluid.  It  is  com 
posed  of  a  glass  tube,  drawn  out  to  a  point,  with  a  small 
orifice.  This  tube  passes  through  the  cork  of  the  bottle. 
By  pressing  in  the  cork  into  the  neck  of  the  bottle,  the  air 
within  will  be  compressed,  and  the  liquid  will  rise  in  the  tube. 
If  now  we  draw  the  cork  out,  with  the  tube  filled  with  the 
fluid,  and  pressing  the  finger  upon  the  upper  orifice,  the  fluid 
can  be  forced  out  in  the  smallest  quantity,  even  to  a  fraction 
of  a  drop. 

10.  Tin. — This  metal  is  used  in  the  form  of  foil,  cut  into 
strips  about  half  an  inch  wide.  Tin  is  very  susceptible  of 
oxidation,  and  therefore  deprives  oxidized  substances  of  their 
oxygen  very  quickly,  when  heated  in  contact  with  them.  It 
is  employed  in  blowpipe  analysis,  for  the  purpose  of  producing 
in  glass  beads  a  lower  degree  of  oxidation,  particularly  if  the 
substance  under  examination  contains  only  a  small  portion  of 
such  oxide.  These  oxides  give  a  characteristic  color  to  the 
bead,  and  thus  are  detected.  The  bead  is  heated  upon  char 
coal  in  the  reduction  flame,  with  a  small  portion  of  the  tin, 
whereby  some  of  the  tin  is  melted  and  mixes  with  the  bead. 
The  bead  should  be  reduced  quickly  in  the  reduction  flame,  for 
by  continuing  the  blast  too  great  a  while,  the  oxide  of  tin 
separates  the  other  oxides  in  the  reduced  or  metallic  state, 
while  we  only  require  that  they  shall  only  be  converted  into 
a  sub-oxide,  in  order  that  its  peculiar  color  may  be  recognized 
in  the  bead.  The  addition  of  too  much  tin  causes  the  bead 


42  T  H  E      B  L  O  W  P  I  P  K  . 

to  present  an  unclean  appearance,  and  prevents  the  required 
reaction. 

11.  Silica    (SiO3). — This  acid  does  not  even  expel  carbonic 
acid  in  the  wet  way,  but  in  a  glowing  heat   it  expels  the 
strongest  volatile  acids.     In  blowpipe  analysis,  we  use  it  fused 
with  carbonate  of  soda  to  a  bead,  as  a  test  for  sulphuric  acid, 
and  in  some  cases  for  phosphoric  acid.     Also  with  carbonate 
of  soda  and  borax,  for  the  purpose  of  separating  tin  from 
copper. 

Finely  powdered  quartz  will  answer  these  purposes.  If  it 
cannot  be  procured,  take  well  washed  white  sand  and  mix  it 
with  two  parts  of  carbonate  of  soda  and  two  parts  of  car 
bonate  of  potassa.  Melt  the  materials  together,  pound  up  the 
cooled  mass,  dissolve  in  hot  water,  filter,  add  to  the  filtrate 
hydrochloric  acid,  and  evaporate  to  dryness.  Moisten  the 
dry  residue  with  hydrochloric  acid,  and  boil  in  water.  The 
silica  remains  insoluble.  It  should  be  washed  well,  dried,  and 
heated,  and  then  reduced  to  powder. 

12.  TEST-PAPERS. — (a.)   Blue   Litmus   Paper. — Dissolve  one 
part  of  litmus  in  six  or  eight  parts  of  water,  and  filter.     Divide 
the  filtrate  into  two  parts.     In  one  of  the  parts  neutralize  the 
free  alkali  by  stirring  it  with  a  glass  rod  dipped  in  diluted 
sulphuric  acid,  until  the  fluid  appears  slightly  red.     Then  mix 
the  two  parts  together,  and  draw  slips  of  unsized  paper,  free 
from  alkali,  such  as  fine  filtering  paper.     Hang  these  strips  on 
a  line  to  dry,  in  the  shade  and  free  from  floating  dust.     If  the 
litmus  solution  is  too  light,  it  will  not  give  sufficient  character 
istic  indications,  and  if  too  dark  it  is  not  sensitive  enough. 
The  blue  color  of  the  paper  should  be  changed  to  red,  when 
brought  in  contact  with  a  solution  containing  the  minutest  trace 
of  free  acid  ;  but  it  should  be  recollected  that  the  neutral  salts 
of  the  heavy  metals  produce  the  same  change. 

(b.)  Red  Litmus  Paper. — The  preparation  of  the  red  litmus 
paper  is  similar  to  the  above,  the  acid  being  added  until  a  red 
color  is  obtained.  Reddened  litmus  paper  is  a  very  sensitive 
reagent  for  free  alkalies,  the  carbonates  of  the  alkalies,  alkaline 


I  T  S      U  S  E  .  43 

earths,  sulphides  of  the  alkalies  and  of  the  alkaline  earths,  and 
alkaline  salts  with  weak  acids,  such  as  boracic  acid.  These 
substances  restore  the  original  blue  color  of  the  litmus. 

(c.)  Logwood  Paper. — Take  bruised  logwood,  boil  it  in 
water,  filter,  and  proceed  as  above.  Logwood  paper  is  a  very 
delicate  test  for  free  alkalies,  which  impart  a  violet  tint  to  it. 
It  is  sometimes  used  to  detect  hydrofluoric  acid,  which  changes 
its  color  to  yellow. 

All  the  test-papers  are  to  be  cut  into  narrow  strips,  and 
preserved  in  closely  stopped  vials.  The  especial  employment 
of  the  test-papers  we  shall  allude  to  in  another  place. 


B.    ESPECIAL   REAGENTS. 

13.  Fused  Boracic  Acid  (BO8). — The  commercial  article  is 
sufficiently  pure  for  blowpipe  analysis.     It  is  employed  in  some 
cases  to  detect  phosphoric  acid,  and  also  minute  traces  of 
copper  in  lead  compounds. 

14.  Fluorspar  (CaFl2). — This  substance  should  be  pounded 
fine   and  strongly   heated.      Fluorspar  is   often    mixed  with 
boracic  acid,  which  renders  it  unfit  for  analytical  purposes. 
Such  an  admixture  can  be  detected  if  it  be  mixed  with  bi- 
sulphate  of  potassa,  and  exposed  upon  platinum  wire  to  the 
interior  or  blue  flame.     It  is  soon  fused,  the  boracic  acid  is 
reduced  and  evaporated,  and  by  passing  through  the  external 
flame  it  is  reoxidized,  and  colors  the  flame  green.     We  use 
fluorspar  mixed  with  bisulphate  of  potassa  as  a  test  for  lithia 
and  boracic  acid  in  complicated  compounds. 

15.  Oxalate  of  Nickel   (NiO,   0). — It  is   prepared  by  dis 
solving  the  pure  oxide  of  nickel  in  diluted  hydrochloric  acid. 
Evaporate  to  dryness,  dissolve  in  water,  and  precipitate  with 
oxalate  of  ammonia.     The  precipitate  must  be  washed  with 
caution  upon  a  filter,  and  then  dried.     It  is  employed  in  blow 
pipe  analysis  to  detect  salts  of  potassa  in  the  presence  of 
sodium  and  lithium. 

16.  Oxide  of  Copper  (CuO). — Pure  metallic  copper  is  dis- 


44  THE     BLOWPIPE. 

solved  in  nitric  acid.  The  solution  is  evaporated  in  a  porcelain 
dish  to  dryness,  and  gradually  heated  over  a  spirit-lamp,  until 
the  blue  color  of  the  salt  has  disappeared  and  the  mass  presents 
a  uniform  black  color.  The  oxide  of  copper  so  prepared  must 
be  powdered,  and  preserved  in  a  vial.  It  serves  to  detect,  in 
complicated  compounds,  minute  traces  of  chlorine. 

It.  Antimoniate  of  Potassa  (KO,  SbO6). — Mix  four  parts 
of  the  bruised  metal  of  antimony,  with  nine  parts  of  saltpetre. 
Throw  this  mixture,  in  small  portions,  into  a  red-hot  Hessian 
crucible,  and  keep  it  at  a  glowing  heat  for  awhile  after  all  the 
mixture  is  added.  Boil  the  cooled  mass  with  water,  and  dry 
the  residue.  Take  two  parts  of  this,  and  mix  it  with  one  part 
of  dry  carbonate  of  potassa,  and  expose  this  to  a  red  heat  for 
about  half  an  hour.  Then  wash  the  mass  in  cold  water,  and 
boil  the  residue  in  water  ;  filter,  evaporate  the  filtrate  to  dry- 
ness,  and  then,  with  a  strong  heat,  render  it  free  of  water. 
Powder  it  while  it  is  warm,  and  preserve  it  in  closed  vials.  It 
is  used  for  the  detection  of  small  quantities  of  charcoal  in  com 
pound  substances,  as  it  shares  its  oxygen  with  the  carbonaceous 
matter,  the  antimony  becomes  separated,  and  carbonate  of 
potassa  is  produced,  which  restores  red  litmus  paper  to  blue, 
and  effervesces  with  acids. 

18.  Silver  Foil. — A  small  piece  of  silver  foil  is  used  for  the 
purpose  of  detecting  sulphur  and  the  sulphides  of  the  metals, 
which  impart  a  dark  stain  to  it.     If  no  silver  foil  is  at  hand, 
strips  of  filtering  paper,  impregnated  with  acetate  of  lead,  will 
answer  in  many  cases. 

19.  Nitroprusside  of  Sodium  (Fe'Cy6,  N0»,  2Na).— This  is  a 
very  delicate  test  for  sulphur,  and  was  discovered  by  Dr.  Playfair. 
This  test  has  lately  been  examined  with  considerable  ability  by 
Prof.  J.  W.  Bailey,,  of  West  Point.     If  any  sulphate  or  sulphide 
is  heated  by  the  blowpipe  upon  charcoal  with  the  carbonate 
of  soda,  and  the  fused  mass  is  placed  on  a  watch-glass,  with  a 
little  water,  and  a  small  piece  of  the  nitroprusside  of  sodium 
is  added,  there  will  be  produced  a  splendid  purple  color.     This 
color,  or  reaction,  will  be  produced  from  any  substance  contain- 


I  T  8      U  S  E  .  4:5 

ing  sulphur,  such  as  the  parings  of  the  nails,  hair,  albumen,  etc. 
In  regard  to  these  latter  substances,  the  carbonate  of  soda 
should  be  mixed  with  a  little  starch,  which  will  prevent  the 
loss  of  any  of  the  sulphur  by  oxidation.  Coil  a  piece  of  hair 
around  a  platinum  wire,  moisten  it,  and  dip  it  into  a  mixture 
of  carbonate  of  soda,  to  which  a  little  starch  has  been  added, 
and  then  heat  it  with  the  blowpipe,  when  the  fused  mass  will 
give  with  the  nitroprusside  of  sodium  the  characteristic  purple 
reaction,  indicative  of  the  presence  of  sulphur.  With  the 
proper  delicacy  of  manipulation,  a  piece  of  hair,  half  an  inch  in 
length,  will  give  distinct  indications  of  sulphur. 

Preparation. — The  nitroprussides  of  sodium  and  potassium 
(for  either  salt  will  give  the  above  reactions),  are  prepared  as 
follows  :  One  atom  (422  grains)  of  pulverized  ferrocyanide  of 
potassium  is  mixed  with  five  atoms  of  commercial  nitric  acid, 
diluted  with  an  equal  quantity  of  water.  One-fifth  of  this 
quantity  (one  atom)  of  the  acid  is  sufficient  to  transfer  the 
ferrocyanide  into  nitroprusside  ;  but  the  use  of  a  larger  quan 
tity  is  found  to  give  the  best  results.  The  acid  is  poured  all  at 
once  upon  the  ferrocyanide,  the  cold  produced  by  the  mixing 
being  sufficient  to  moderate  the  action.  The  mixture  first 
assumes  a  milky  appearance,  but  after  a  little  while,  the  salt 
dissolves,  forming  a  coffee-colored  solution,  and  gases  are 
disengaged  in  abundance.  When  the  salt  is  completely  dis 
solved,  the  solution  is  found  to  contain  ferrocyanide  (red 
prussiate)  of  potassium,  mixed  with  nitroprusside  and  nitrate 
of  the  same  base.  It  is  then  immediately  decanted  into  a 
large  flask,  and  heated  over  the  water-bath.  It  continues 
to  evolve  gas,  and  after  awhile,  no  longer  yields  a  dark 
blue  precipitate  with  ferrous  salts,  but  a  dark  green  or  slate- 
colored  precipitate.  It  is  then  removed  from  the  fire,  and  left 
to  crystallize,  whereupon  it  yields  a  large  quantity  of  crystals 
of  nitre,  and  more  or  less  oxamide.  The  strongly-colored  mother 
liquid  is  then  neutralized  with  carbonate  of  potash  or  soda, 
according  to  the  salt  to  be  prepared,  and  the  solution  is  boiled, 
whereupon  it  generally  deposits  a  green  or  brown  precipitate, 


46  THE    BLOWPIPE. 

which  must  be  separated  by  filtration.  The  liquid  then  con 
tains  nothing  but  nitroprusside  and  nitrate  of  potash  or  soda. 
The  nitrates  being  the  least  soluble,  are  first  crystallized, 
and  the  remaining  liquid,  on  farther  evaporation,  yields  crys 
tals  of  the  nitroprusside.  The  sodium  salt  crystallizes  most 
easily. — (  PLAYFAIR.  ) 

As  some  substances,  particularly  in  complicated  compounds, 
a,re  not  detected  with  sufficient  nicety  in  the  dry  way  of  ana 
lysis,  it  will  often  be  necessary  to  resort  to  the  wet  way.  It  is 
therefore  necessary  to  have  prepared  the  reagents  required 
for  such  testing,  as  every  person,  before  he  can  become  an 
expert  blowpipe  analyst,  must  be  acquainted  with  the  charac 
teristic  tests  as  applied  in  the  wet  way. 


Part    II. 


INITIATORY  ANALYSIS. 

QUALITATIVE  ANALYSIS  refers  to  those  examinations  which 
relate  simply  to  the  presence  or  the  absence  of  certain  sub. 
stances,  irrespective  of  their  quantities.  But  before  we  take 
cognizance  of  special  examinations,  it  would  facilitate  the 
progress  of  the  student  to  pass  through  a  course  of  Initiatory 
Exercises.  These  at  once  lead  into  the  special  analysis  of 
all  those  substances  susceptible  of  examination  by  the  blowpipe. 
The  Initiatory  Analysis  is  best  studied  by  adopting  the  following 
arrangement : 

1.  Examinations  with  the  glass  bulb. 


with  the  open  tube. 

upon  charcoal. 

in  the  platinum  forceps. 

in  the  borax  bead. 

in  microcosmic  salt. 

in  the  carbonate  of  soda  bead. 


8.  Confirmatory  examinations. 

1.    EXAMINATIONS    WITH   THE    GLASS    BULB. 

The  glass  of  which  the  bulb  is  made  should  be  entirely  free 
from  lead,  otherwise  fictitious  results  will  ensue.     If  the  bulb 

^-^  47 


48  THE     BLOWPIPE. 

be  of  flint  glass,  then  by  heating  it,  there  is*  a  slightly  iridescent 
film  caused  upon  the  surface  of  the  glass,  which  may  easily  be 
mistaken  for  arsenic.  Besides,  this  kind  of  glass  is  easily  fusible 
in  the  oxidating  flame  of  the  blowpipe,  while,  in  the  reducing 
flame,  its  ready  decomposition  would  preclude  its  use  entirely. 
The  tube  should  be  composed  of  the  potash  or  hard  Bohemian 
glass,  should  be  perfectly  white,  and  very  thin,  or  the  heat  will 
crack  it. 

The  tube  should  be  perfectly  clean,  which  can  be  easily 
attained  by  wrapping  a  clean  cotton  rag  around  a  small  stick, 
and  inserting  it  in  the  tube.  Before  using  the  tube,  see  also 
that  it  is  perfectly  dry. 

The  quantity  of  the  substance  put  into  the  tube  for  exami 
nation  should  be  small.  From  one  to  three  grains  is  quite 
sufficient,  as  a  general  rule,  but  circumstances  vary  the  quantity. 
The  sides  of  the  tube  should  not  catch  any  of  the  substance  as 
it  is  being  placed  at  the  bottom  of  the  tube,  or  into  the  bulb. 
If  any  of  the  powder,  however,  should  adhere,  it  should  be 
pushed  down  with  a  roll  of  clean  paper,  or  the  clean  cotton 
rag  referred  to  above. 

In  submitting  the  tube  to  the  flame,  it  should  be  heated  at 
first  very  gently,  the  heat  being  increased  until  the  glass  begins 
to  soften,  when  the  observations  of  what  is  ensuing  within  it 
may  be  made. 

If  the  substance  be  of  an  organic  nature,  a  peculiar  empy. 
reumatic  odor  will  be  given  off.  If  the  substance  chars,  then 
it  may  be  inferred  that  it  is  of  an  organic  nature.  The  matters 
which  are  given  off  and  cause  the  empyreumatic  odor,  are  a 
peculiar  oil,  ammonia,  carbonic  acid,  acetic  acid,  water,  cyano 
gen,  and  frequently  other  compounds.  If  a  piece  of  paper  is 
heated  in  the  bulb,  a  dark  colored  oil  condenses  upon  the  sides 
of  the  tube,  which  has  a  strong  empyreumatic  odor.  A  piece 
of  litmus  paper  indicates  that  this  oil  is  acid,  as  it  is  quickly 
changed  to  red  by  contact  with  it.  A  black  residue  is  now 
left  in  the  tube,  and  upon  examination  we  will  find  that  it  is 
charcoal.  If,  instead  of  the  paper,  a  piece  of  animal  substance 


INITIATORY     ANALYSIS.  49 

is  placed  m  the  bulb,  the  reddened  litmus  paper  will  be  con 
verted  into  its  original  blue  color,  while  charcoal  will  be  left 
at  the  bottom  of  the  tube. 

A  changing  of  the  substance,  however,  to  a  dark  color, 
should  not  be  accepted  as  an  invariable  indication  of  charcoal, 
as  some  inorganic  bodies  thus  change  color,  but  the  dark 
substance  will  not  be  likely  to  be  mistaken  for  charcoal.  By 
igniting-  the  suspected  substance  with  nitrate  of  potassa,  it  can 
quickly  be  ascertained  whether  it  is  organic  or  not,  for  if  the 
latter,  the  vivid  deflagration  will  indicate  it. 

If  the  substance  contains  water,  it  will  condense  upon  the 
cold  portion  of  the  tube,  and  may  be  there  examined  as  to 
whether  it  is  acid  or  alkaline.  If  the  former,  the  matter  under 
examination  is,  perhaps,  vegetable  ;  if  the  latter,  it  is  of  an 
animal  nature.  The  water  may  be  that  fluid  absorbed,  or  it 
may  form  a  portion  of  its  constitution. 

If  the  substance  contain  sulphur,  the  sublimate  upon  the 
cold  part  of  the  tube  may  be  recognized  by  its  characteristic 
appearance,  especially  if  the  substance  should  be  a  sulphide  of 
tin,  copper,  antimony,  or  iron.  The  hyposulphites,  and  several 
other  sulphides,  also  give  off  sulphur  when  heated.  The 
volatile  metals,  mercury  and  arsenic,  will,  however,  sublime 
without  undergoing  decomposition.  As  the  sulphide  of  arsenic 
may  be  mistaken,  from  its  color  and  appearance,  for  sulphur, 
it  must  be  examined  especially  for  the  purpose  of  determining 
that  point. 

Selenium  will  likewise  sublime  by  heat  as  does  sulphur.  This 
is  the  case  if  selenides  are  present.  Selenium  gives  off  the 
smell  of  decayed  horse-radish. 

When  the  persalts  are  heated  they  are  reduced  to  protosalts, 
with  the  elimination  of  a  part  of  their  acid.  This  will  be 
indicated  by  the  blue  litmus  paper. 

If  some  of  the  neutral  salts  containing  a  volatile  acid  be 
present,  they  will  become  decomposed.  For  instance,  the  red 
nitrous  acid  water  of  the  nitrates  will  indicate  the  decomposition 
of  the  salt,  especially  if  it  be  the  nitrate  of  a  metalic  oxide. 

3 


50  T  H  E     BLOWPIPE. 

If  there  is  an  odor  of  sulphur,  then  it  is  quite  probable,  if 
no  free  sulphur  be  present,  that  a  hyposulphite  is  decomposed. 

If  an  oxalate  be  present,  it  is  decomposed  with  the  evolution 
of  carbonic  oxide,  which  may  be  inflamed  at  the  mouth  of  the 
tube  ;  but  there  are  oxalates  that  give  t)ff  carbonic  acid  gas, 
which,  of  course,  will  not  burn.  A  cyanide  will  become  decom 
posed  and  eliminate  nitrogen  gas,  while  the  residue  is  charred. 
Some  cyanides  are,  however,  not  thus  decomposed,  as  the  dry 
cyanides  of  the  earths  and  alkalies. 

There  are  several  oxides  of  metals  which  will  sublime,  and 
may  be  thus  examined  in  the  tube.  Arsenious  acid  sublimes  with 
great  ease  in  minute  octohedral  crystals.  The  oxides  of  tellu 
rium  and  antimony  will  sublime,  the  latter  in  minute  glittering 
needles. 

There  are  several  metals  which  will  sublime,  and  may  be 
examined  in  the  cold  portion  of  the  tube.  Mercury  condenses 
upon  the  tube  in  minute  globules.  These  often  do  not  present 
the  metalic  appearance  until  they  are  disturbed  with  a  glass 
rod,  when  they  attract  each  other,  and  adhere  as  small 
globules.  Place  in  the  tube  about  a  grain  of  red  precipitate 
of  the  drug  stores  and  apply  heat,  when  the  oxide  will  become 
decomposed,  its  oxygen  will  escape  while  the  vaporized  mer 
cury  will  condense  upon  the  cold  portion  of  the  tube,  and  may 
tfcere  be  examined  with  a  magnifying  glass. 

'Arsenic,  when  vaporized,  may  be  known  by  its  peculiar  alli 
aceous  odor.  Arsenic  is  vaporized  from  its  metallic  state,  and 
likewise  from  its  alloys.  Several  compounds  which  contain 
arsenic  will  also  sublime,  such  as  the  arsenical  cobalt.  Place 
in  the  bulb  a  small  piece  of  arsenical  cobalt  or  "fly-stone," 
and  apply  heat.  The  sulphide  of  arsenic  will  first  rise,  but 
soon  the  arsenic  will  adhere  to  the  sides  of  the  tube. 

The  metals  tellurium  and  cadmium  are  susceptible  of  solution, 
but  the  heat  required  is  a  high  one.  This  is  best  done  upon 
charcoal. 

The  perchloridc  of  mercury  sublimes  undecomposed  in  the  bulb, 
previously  undergoing  fusion. 


INITIATORY     ANALYSIS.  51 

The  prutockloride  of  mercury  likewise  sublimes,  but  it  docs  not 
undergo  fusion  first,  as  is  the  case  with  the  corrosive  sublimate. 

The  ammoniacal  salts  all  are  susceptible  of  sublimation,  which 
they  do  without  leaving  a  residue.  There  are,  however,  several 
which  contain  fixed  *acids,  which  latter  are  left  in  the  bulb. 
This  is  particularly  the  case  with  the  phosphates  and  borates 
A  piece  of  red  litmus  paper  will  readily  detect  the  escaping 
ammonia,  while  its  odor  will  indicate  its  presence  with  great 
certainty.  The  halogen  compounds  of  mercury,  we  should  have 
mentioned,  also  sublime,  the  red  iodide  giving  a  yellow  subli 
mate. 

The  bulb  is  also  a  convenient  little  instrument  for  the  pur 
pose  of  heating  those  substances  which  phosphoresce,  and  like 
wise  those  salts  that  decrepitate. 

Should  the  above  reactions  not  be  readily  discerned,  it  should 
not  be  considered  as  an  indication  that  the  substances  are  not 
present,  for  they  are  frequently  expelled  in  such  combinations 
that  the  above  reactions  will  not  take  place.  This  is  often  tho 
case  with  sulphur,  selenium,  arsenic,  and  tellurium.  It  fre 
quently  happens,  likewise,  that  these  substances  are  in  such 
combinations  that  heat  alone  will  not  sublime  them  ;  or  else  two 
or  more  of  them  may  arise  together,  and  thus  complicate  the 
sublimate,  so  that  the  eye  cannot  readily  detect  either  substance. 
Sometimes  sulphur  and  arsenic  will  coat  the  tube  with  a  metal- 
like  appearance,  which  is  deceptive.  This  coating  presents  a 
metallic  lustre  at  its  lower  portion,  but  changing,  as  it  pro 
gresses  upward,  to  a  dark  brown,  light  brown,  orange  or  yellow  ; 
this  sublimate  being  due  to  combinations  of  arsenic  and  sulphur, 
which  compounds  are  volatilized  at  a  lower  temperature  than 
metallic  arsenic. 

If  certain  reagents  are  mixed  with  many  substances,  changes 
are  effected  which  would  not  ensue  with  heat  alone.  Formiote 
of  soda  possesses  the  property  of  readily  reducing  metallic 
oxides.  When  this  salt  is  heated,  it  gives  off  a  quantity  of 
carbonic  oxide  gas.  This  gas,  when  in  the  presence  of  a  metal 
lic  oxide,  easily  reduces  the  metal,  by  withdrawing  its  oxygen 


52  THE     BLOWPIPE. 

from  it,  and  being  changed  into  carbonic  oxide.  If  a  little  fly- 
stone  is  mixed  with  some  formiate  of  soda,  and  heated  in  the 
bulb,  the  arsenic  is  reduced,  volatilized,  and  condenses  in  the 
cool  portion  of  the  tube.  By  this  method,  the  smallest  portion 
of  a  grain  of  the  arsenical  compound  may  be  thus  examined 
with  the  greatest  readiness.  If  the  residue  is  now  washed,  by 
which  the  soda  is  got  rid  of,  the  metallic  arsenic  may  be  obtained 
in  small  spangles.  If  the  compound  examined  be  the  sulphide 
of  antimony,  the  one-thousandth  part  can  be  readily  detected,  and 
hence  this  method  is  admirably  adapted  to  the  examination  of 
medicinal  antimonial  compounds.  The  arsenites  of  silver  and  cop 
per  are  reduced  by  the  formiate  of  soda  to  their  metals,  mixed  with 
metallic  arsenic.  The  mercurial  salts  are  all  reduced  with  the 
metal  plainly  visible  as  a  bright  silvery  ring  on  the  cool  por 
tion  of  the  tube.  The  chloride  and  nitrate  of  silver  are  com 
pletely  reduced,  and  may  be  obtained  after  working  out  the 
soda,  as  bright  metallic  spangles.  The  salts  of  antimony  and 
zinc  are  thus  reduced  ;  also  the  sulphate  of  cadmium.  The 
sublimate  of  the  latter,  although  in  appearance  not  unlike  that 
of  arsenic,  can  easily  be  distingushed  by  its  brighter  color.  It 
is,  in  fact,  the  rich  yellow  of  this  sublimate  which  has  led  artists 
to  adopt  it  as  one  of  their  most  valued  pigments. 

2.    EXAMINATIONS    IN   THE    OPEN   TUBE. 

The  substance  to  be  operated  upon  should  be  placed  in  the 
tube,  about  half  an  inch  from  the  end,  and  the  flame  applied  at 
first  very  cautiously,  increasing  gradually  to  the  required  tempe 
rature.  The  tube,  in  all  these  roasting  operations,  as  they  are 
termed,  should  be  held  in  an  inclined  position.  The  nearer 
perpendicular  the  tube  is  held,  the  stronger  is  the  draught  of 
air  that  passes  through  it.  If  but  little  heat  is  required  in  the 
open  tube  operation,  the  spirit-lamp  is  the  best  method  of 
applying  the  heat.  But  if  a  greater  temperature  is  required, 
then  recourse  must  be  had  to  the  blowpipe.  Upon  the  angle 
of  inclination  of  the  tube  depends  the  amount  of  air  that  passes 


I  N  i  T  i  A  T  o  K  Y     ANALYSIS. 


53 


through  it,  and  therefore,  the  rapidity  of  the  draught  may  be 
easily  regulated  at  the  will  of  the  operator.  The  inclination  of 
the  tube  may,  as  a  general  rule,  be  about  the  angle  represented 
in  Fisr  14. 


Fig.  14. 


The  length  of  the  tube  must  be  about  six  inches,  so  that  the 
portion  upon  which  the  substance  rested  in  a  previous  examina 
tion  may  be  cut  off.  The  portion  of  the  tube  left  will  answer 
for  several  similar  operations. 

When  the  substance  is  under  examination,  we  should  devote 
our  attention  to  the  nature  of  the  sublimates,  and  to  that  of 
the  odors  of  the  gases.  If  sulphur  be  in  the  substance  experi 
mented  upon,  the  characteristic  odor  of  sulphurous  acid  gas  will 
readily  indicate  the  sulphur.  If  metallic  sulphides,  for  instance, 
are  experimented  upon,  the  sulphurous  acid  gas  eliminated  will 
readily  reveal  their  presence.  As  it  is  a  property  of  this  gas 
to  bleach,  a  piece  of  Brazil-wood  test  paper  should  be  held  in 
the  mouth  of  the  tube,  when  its  loss  of  color  will  indicate  the 
presence  of  the  sulphurous  acid.  It  often  happens,  too,  that  a 
slight  deposition  of  sulphur  will  be  observed  upon  the  cool  por- 


54:  THE     BLOWPIPE. 

tion  of  the  tube.  This  is  particularly  the  case  with  those  sul 
phides  which  yield  sublimates  of  sulphur  when  heated  in  the 
bulb. 

Selenium  undergoes  but  slight  oxidation,  but  it  becomes 
readily  volatilized,  and  may  be  observed  on  the  cool  portion 
of  the  tube.  At  the  same  time  the  nose,  if  applied  close  to  the 
end  of  the  tube,  will  detect  the  characteristic  odor  of  rotten 
horse-radish.  Arsenic  also  gives  its  peculiar  alliaceous  odor, 
which  is  so  characteristic  that  it  can  be  easily  detected.  A 
few  of  the  arsenides  produce  this  odor.  The  sublimates  should 
be  carefully  observed,  as  they  indicate  often  with  great  cer 
tainty  the  presence  of  certain  substances  ;  for  instance,  that 
of  arsenic.  The  sublimate,  in  this  case,  presents  itself  as  the 
arsenious  acid,  or  the  metallic  arsenic  itself.  If  it  be  the  former, 
it  may  be  discerned  by  aid  of  the  magnifying  glass  as  beauti 
ful  glittering  octohedral  crystals.  If  the  latter,  the  metallic 
lustre  will  reveal  it. 

But  it  will  be  observed  that  while  some  of  the  arsenides  are 
sublimed  at  a  comparatively  low  temperature,  others  require 
a  very  high  one. 

Antimony  gives  a  white  sublimate  when  its  salts  are  roasted, 
as  the  sulphide,  or  the  antimonides  themselves,  or  the  oxide  of 
this  metal.  This  white  sublimate  is  not  antimonious  acid,  but 
there  is  mixed  with  it  the  oxide  of  antimony  with  which  the 
acid  is  sublimed.  As  is  the  case  with  arsenious  acid,  the  anti 
monious  acid  may,  by  dexterous  heating,  be  driven  from  one 
portion  of  the  tube  to  another. 

Tellurium,  or  its  acid  and  oxide,  may  be  got  as  a  sublimate 
in  the  tube.  The  tellurious  acid,  unlike  the  arsenious  and  anti 
monious  acids,  cannot  be  driven  from  one  portion  of  the  tube 
to  another,  but,  on  the  contrary,  it  fuses  into  small  clear 
globules,  visible  to  the  naked  eye  sometimes,  but  quite  so  with 
the  aid  of  the  magnifying  glass. 

Lead,  or  its  chloride,  sublimes  like  tellurium,  and,  like  that 
substance,  fuses  into  globules  or  drops. 

Bismuth,  or  its  sulphide,  sublimes  into  an  orange  or  brown- 


INITIATORY     ANALYSIS.  55 

Ish  globules,  when  it  is  melted,  as  directed  •  above,  for  tellu 
rium.  The  color  of  the  bismuth  and  lead  oxides  are  somewhat 
similar,  although  that  of  the  latter  is  paler. 

If  any  mineral  containing  fluorine  is  fused,  first  with  the 
microcosmic  salt  bead,  then  put  into  the  tube,  and  the  flame 
of  the  blowpipe  be  directed  into  the  tube  upon  the  bead,  hydro 
fluoric  acid  is  disengaged  and  attacks  the  inside  of  the  tube. 
The  fluoride  of  calcium,  or  fluorspar,  may  be  used  for  this 
experiment. 

During  the  roasting,  a  brisk  current  of  air  should  be  allowed 
to  pass  through  the  tube,  whereby  unoxidized  matter  may  be 
prevented  from  volatilization,  and  the  clogging  up  of  the  sub 
stance  under  examination  be  prevented. 

3.    EXAMINATIONS    UPON    CHARCOAL. 

In  making  examinations  upon  charcoal,  it  is  quite  necessary 
that  the  student  should  make  himself  familiar  with  the  different 
and  characteristic  appearances  of  the  deposits  upon  the  char 
coal.  In  this  case  I  have  found  the  advice  given  by  Dr.  Sherer 
to  be  the  best ;  that  is,  to  begin  with  the  examination  of  the 
pure  materials  first,  until  the  eye  becomes  familiarized  with  the 
appearances  of  their  incrustations  upon  charcoal. 

The  greater  part  of  the  metals  fuse  when  submitted  to  the 
heat  of  the  blowpipe,  and  if  exposed  to  the  outer  flame,  they 
oxidize.  These  metals,  termed  the  noble  metals,  do  not  oxidize, 
but  they  fuse.  The  metals  platinum,  iridium,  rhodium,  osmium 
and  palladium  do  not  fuse.  The  metal  osmium,  if  exposed  to 
the  flame  of  oxidation,  fuses  and  is  finally  dissipated  as  osmic 
acid.  In  the  latter  flame,  the  salts  of  the  noble  metals  are 
reduced  to  the  metallic  state,  and  the  charcoal  is  covered  with 
the  bright  metal. 

We  shall  give  a  brief  description  of  the  appearance  of  the 
principal  elementary  bodies  upon  being  fused  with  charcoal. 
This  plan  is  that  deemed  the  most  conducive  to  the  progress 
of  the  student,  by  Berzelius,  Plattner,  and  Sherer.  Experience 


56  THE     B  L  o  w  P  i  P  E  . 

has  taught  us  that  this  method  is  the  most  efficient  that  could 
have  been  devised  as  an  initiatory  exercise  for  the  student,  ere 
he  commences  a  more  concise  and  methodical  method  of  analy 
sis.  In  these  reactions  upon  charcoal,  we  shall  follow  nearly 
the  language  of  Plattner  and  Sherer. 

SELENIUM  is  not  difficult  of  fusion,  and  gives  off  brown  fumes 
in  either  the  oxidation  or  reduction  flame.  The  deposit  upon  the 
charcoal  is  of  a  steel-grey  color,  with  a  slightly  metallic  lustre. 
The  deposit  however  that  fuses  outside  of  this  steel-grey  one  is 
of  a  dull  violet  color,  shading  off  to  a  light  brown.  Under  the 
flame  of  oxidation  this  deposit  is  easily  driven  from  one  portion 
of  the  charcoal  to  another,  while  the  application  of  the  re 
ducing  flame  volatilizes  it  with  the  evolution  of  a  beautiful 
blue  light.  The  characteristic  odor  of  decayed  horse-radish 
distinguishes  the  volatilization  of  this  metal. 

TELLURIUM. — This  metal  fuses  with  the  greatest  readiness, 
and  is  reduced  to  vapor  under  both  flames  with  fumes,  and 
coats  the  charcoal  with  a  deposit  of  tellurous  acid.  This 
deposit  is  white  near  the  centre,  and  is  of  a  dark  yellow  near 
the  edges.  It  may  be  driven  from  place  to  place  by  the  flame 
of  oxidation,  while  that  of  reduction  volatilizes  it  with  a  green 
flame.  If  there  be  a  mixture  of  selenium  present,  then  the 
color  of  the  flame  is  bluish-green. 

ARSENIC. — This  metal  is  volatilized  without  fusing,  and 
covers  the  charcoal  both  in  the  oxidizing  and  reducing  flames 
with  a  deposit  of  arsenious  acid.  This  coating  is  white  in  the 
centre,  and  grey  towards  the  edges,  and  is  found  some  distance 
from  the  assay.  By  the  most  gentle  application  of  the  flame, 
it  is  immediately  volatilized,  and  if  touched  for  a  moment  with 
the  reducing  flame,  it  disappears,  tinging  the  flame  pale  blue. 
During  volatilization  a  strong  garlic  odor  is  distincly  percepti 
ble,  very  characteristic  of  arsenic,  and  by  which  its  presence 
in  any  compound  may  be  immediately  recognized. 

ANTIMONY. — This  metal  fuses  readily,  and  coats  the  charcoal 
under  both  flames  with  antimonious  acid.  This  incrustation  is 
of  a  white  color  where  thick,  but  of  a  bluish  tint  where  it  is 


INITIATORY    ANALYSIS.  57 

thin,  and  is  found  nearer  to  the  assay  than  that  of  arsenic. 
When  greatly  heated  by  the  flame  of  oxidation,  it  is  driven 
from  place  to  place  without  coloring  the  flame,  but  when  vola 
tilized  by  the  flame  of  reduction,  it  tinges  the  flame  blue.  As 
antimonious  acid  is  not  so  volatile  as  arsenious  acid,  they  may 
thus  be  easily  distinguished  from  one  another. 

When  metallic  antimony  is  fused  upon  charcoal,  and  the 
metallic  bead  raised  to  a  red  heat,  if  the  blast  be  suspended, 
the  fluid  bead  remains  for  some  time  at  this  temperature,  giving 
off  opaque  white  fumes,  which  are  at  first  deposited  on  the 
surrounding  charcoal,  and  then  upon  the  bead  itself,  covering 
it  with  white,  pearly  crystals.  The  phenomenon  is  dependent 
upon  the  fact,  that  the  heated  button  of  antimony,  in  absorbing 
oxygen  from  the  air,  developes  sufficient  heat  to  maintain  the 
metal  in  a  fluid  state,  until  it  becomes  entirely  covered  with 
crystals  of  antimonious  acid  so  formed. 

BISMUTH. — This  metal  fuses  with  ease,  and  under  both  flames 
covers  the  charcoal  with  a  coating  of  oxide,  which,  while  hot, 
is  of  an  orange-yellow  color,  and  after  cooling,  of  a  lemon-yel 
low  color,  passing,  at  the  edges,  into  a  bluish  white.  This 
white  coating  consists  of  the  carbonate  of  bismuth.  The  subli 
mate  from  bismuth  is  formed  at  a  less  distance  from  the  assay 
than  is  the  case  with  antimony.  It  may  be  driven  from  place 
to  place  by  the  application  of  either  flame  ;  but  in  so  doing, 
the  oxide  is  first  reduced  by  the  heated  charcoal,  and  the 
metallic  bismuth  so  formed  is  volatilized  and  reoxidized.  The 
flame  is  uncolored. 

LEAD. — This  metal  readily  fuses  under  either  flame,  and 
incrusts  the  charcoal  with  oxide  at  about  the  same  distance 
from  the  assay  as  is  the  case  with  bismuth.  The  oxide  is,  while 
hot,  of  a  dark  lemon-yellow  color,  but  upon  cooling,  becomes 
of  a  sulphur  yellow.  The  carbonate  which  is  formed  upon  the 
charcoal,  beyond  the  oxide,  is  of  a  bluish-white  color.  If  the 
yellow  incrustation  of  the  oxide  be  heated  with  the  flame  of 
oxidation,  it  disappears,  undergoing  changes  similar  to  those  of 

3* 


58  THE     BLOW  PIPE. 

bismuth  above  mentioned.  Under  the  flame  of  reduction,  it, 
however,  disappears,  tinging  the  flame  blue. 

CADMIUM. — This  metal  fuses  with  ease,  and,  in  the  flame  of 
oxidation,  takes  fire,  and  burns  with  a  deep  yellow  color,  giving 
off  brown  fumes,  which  coat  the  charcoal,  to  within  a  small 
distance  of  the  assay,  with  oxide  of  cadmium.  This  coating 
exhibits  its  characteristic  reddish-brown  color  most  clearly  when 
cold.  Where  the  coating  is  very  thin,  it  passes  to  an  orange 
color.  As  oxide  of  cadmium  is  easily  reduced,  and  the  metal 
very  volatile,  the  coating  of  oxide  may  be  driven  from  place  to 
place  by  the  application  of  either  flame,  to  neither  of  which 
does  it  impart  any  color.  Around  the  deposit  of  oxide,  the 
charcoal  has  occasionally  a  variegated  tarnish. 

ZINC. — This  metal  fuses  with  ease,  and  takes  fire  in  the  flame 
of  oxidation,  burning  with  a  brilliant  greenish-white  light,  and 
forming  thick  white  fumes  of  oxide  of  zinc,  which  coat  the 
charcoal  round  the  assay.  This  coating  is  yellow  while  hot, 
but  when  perfectly  cooled,  becomes  white.  If  heated  with  the 
flame  of  oxidation,  it  shines  brilliantly,  but  is  not  volatilized, 
since  the  heated  charcoal  is,  under  these  circumstances,  insuffi 
cient  to  effect  its  reduction.  Even  under  the  reducing  flame, 
it  disappears  very  slowly. 

TIN. — This  metal  fuses  readily,  and,  in  the  flame  of  oxidation, 
becomes  covered  with  oxide,  which,  by  a  strong  blast,  may 
be  easily  blown  off.  In  the  reducing  flame,  the  fused  metal 
assumes  a  white  surface,  and  the  charcoal  becomes  covered  with 
oxide.  This  oxide  is  of  a  pale  yellow  color  while  hot,  and  is 
quite  brilliant  when  the  flame  of  oxidation  is  directed  upon 
it.  After  cooling,  it  becomes  white.  It  is  found  immediately 
around  the  assay,  and  cannot  be  volatilized  by  the  application 
of  either  flame. 

MOLYBDENUM. — This  metal,  in  powder,  is  infusible  before  the 
blowpipe.  If  heated  in  the  outer  flame,  it  becomes  gradually 
oxidized,  and  incrusts  the  charcoal,  at  a  small  distance  from 
the  assay,  with  molybdic  acid,  which,  near  the  assay,  forms 


INITIATORY     ANALYSIS.  59 

transparent  crystalline  scales,  and  is  elsewhere  deposited  as  a 
fine  powder.  The  incrustation,  while  hot,  is  of  a  yellow  color, 
but  becomes  white  after  cooling.  It  may  be  volatilized  by 
heating  with  either  flame,  and  leaves  the  surface  of  the  char 
coal,  when  perfectly  cooled,  of  a  dark-red  copper  color,  with  a 
metallic  lustre,  due  to  the  oxide  of  molybdenum,  which  has  been 
formed  by  the  reducing  action  of  the  charcoal  upon  the  molyb. 
die  acid.  In  the  reducing  flame,  metallic  molybdenum  remains 
unchanged. 

SILVER. — This  metal,  when  fused  alone,  and  kept  in  this 
state  for  some  time,  under  a  strong  oxidizing  flame,  covers  the 
charcoal  with  a  thin  film  of  dark  reddish-brown  oxide.  If  the 
silver  be  alloyed  with  lead,  a  yellow  incrustation  of  the  oxide 
of  that  metal  is  first  formed,  and  afterwards,  as  the  silver 
becomes  more  pure,  a  dark  red  deposit  is  formed  on  the  char 
coal  beyond.  If  the  silver  contains  a  small  quantity  of  anti 
mony,  a  white  incrustation  of  antimonious  acid  is  formed,  which 
becomes  red  on  the  surface  if  the  blast  be  continued.  And  if 
lead  and  antimony  are  both  present  in  the  silver,  after  the  greater 
part  of  these  metals  have  been  volatilized,  a  beautiful  crimson 
incrustation  is  produced  upon  the  charcoal.  This  result  is 
sometimes  obtained  in  fusing  rich  silver  ores  on  charcoal. 

SULPHIDES,    CHLORIDES,    IODIDES,    AND    BROMIDES. 

In  blowpipe  experiments,  it  rarely  occurs  that  we  have  to 
deal  with  pure  metals,  which,  if  not  absolutely  non-volatile, 
are  recognized  by  the  incrustation  they  form  upon  charcoal. 
Some  compound  substances,  when  heated  upon  charcoal,  form 
white  incrustations,  resembling  that  formed  by  antimony,  and 
which,  when  heated,  may,  in  like  manner,  be  driven  from  place 
to  place.  Among  these  are  certain  sulphides,  as  sulphide  of 
potassium,  and  sulphide  of  sodium,  which  are  formed  by  the 
action  of  the  reducing  flame  upon  the  sulphates  of  potassa  and 
soda,  and  are,  when  volatilized,  reconverted  into  those  sulphates, 
and  as  such  deposited  on  the  charcoal.  No  incrustation  is, 


60  THE     B  L  o  w  P  i  P  K  . 

however,  foiined,  until  the  whole  of  the  alkaline  sulphate  has 
been  absorbed  into  the  charcoal,  and  has  parted  with  its  oxy 
gen.  As  sulphide  of  potassium  is  more  volatile  than  sulphide 
of  sodium,  an  incrustation  is  formed  from  the  former  sooner 
than  from  the  latter  of  these  salts,  and  is  considerably  thicker 
in  the  former  case.  If  the  potash  incrustation  be  touched  witli 
the  reducing  flame,  it  disappears  with  a  violet-colored  flame  ; 
and  if  a  soda  incrustation  be  treated  in  like  manner,  an  orange- 
yellow  flame  is  produced. 

Sulphide  of  lithium,  formed  by  heating  the  sulphate  in  the 
reducing  flame,  is  volatilized  in  similar  manner  by  a  strong 
blast,  although  less  readily  than  the  sulphide  of  sodium.  It 
affords  a  greyish  white  film,  which  -disappears  with  a  crimson 
flame  when  submitted  to  the  reducing  flame. 

Besides  the  above,  the  sulphides  of  bismuth  and  lead  give, 
when  heated  in  either  flame,  two  different  incrustations,  of 
which  the  more  volatile  is  of  a  white  color,  and  consists  in  the 
one  case  of  sulphate  of  lead,  and  in  the  other  of  sulphate  of 
bismuth.  If  either  of  these  be  heated  under  the  reducing  flame, 
it  disappears  in  the  former  case  with  a  bluish  flame,  in  the 
latter  unaccompanied  by  any  visible  flame.  The  incrustation 
formed  nearest  to  the  assay  consists  of  the  oxide  of  lead  or 
bismuth,  and  is  easily  recognized  by  its  color  when  hot  and 
after  cooling.  There  are  many  other  metallic  sulphides,  which, 
when  heated  by  the  blowpipe  flame,  cover  the  charcoal  with 
a  white  incrustation,  as  sulphide  of  antimony,  sulphide  of  zinc, 
and  sulphide  of  tin.  In  all  these  cases,  however,  the  incrusta 
tion  consists  of  the  metallic  oxide  alone,  and  either  volatilizes 
or  remains  unchanged,  when  submitted  to  the  oxidizing  flame. 

Of  the  metallic  chlorides  there  are  many  which,  when  heated 
on  charcoal  with  the  blowpipe  flame,  are  volatilized  and  re- 
deposited  as  a  white  incrustation.  Among  these  are  the 
chlorides  cf  potassium,  sodium,  and  lithium,  which  volatilize 
and  cover  the  charcoal  immediately  around  the  assay  with  a 
thin  white  film,  after  they  have  been  fused  and  absorbed  into 
the  charcoal,  chloride  of  potassium  forms  the  thickest  de 


INITIATORY     ANALYSIS.  61 

and  chloride  of  lithium  the  thinnest,  the  latter  being  moreover 
of  a  greyish- white  color.  The  chlorides  of  ammonium,  mercury, 
and  antimony  volatilize  without  fusing. 

The  chlorides  of  zinc,  cadmium,  lead,  bismuth,  and  tin  first 
fuse  and  then  cover  the  charcoal  with  two  different  incrusta 
tions,  one  of  which  is  a  white  volatile  chloride,  and  the  other 
a  less  volatile  oxide  of  the  metal. 

Some  of  the  incrustations  formed  by  metallic  chlorides  dis. 
appear  with  a  colored  flame  when  heated  with  the  reducing 
flame  ;  thus  chloride  of  potassium  affords  a  violet  flame,  chlo 
ride  of  sodium  an  orange  one,  chloride  of  lithium  a  crimson 
flame,  and  chloride  of  lead  a  blue  one.  The  other  metals 
mentioned  above  volatilize  without  coloring  the  flame. 

The  chloride  of  copper  fuses  and  colors  the  flame  of  a  beauti 
ful  blue.  Moreover,  if  a  continuous  blast  be  directed  upon  the 
salt,  a  part  of  it  is  driven  off  in  the  form  of  white  fumes  which 
smell  strongly  of  chlorine,  and  the  charcoal  is  covered  with 
incrustations  of  three  different  colors.  That  which  is  formed 
nearest  to  the  assay  is  of  a  dark  grey  color,  the  next,  a  dark 
yellow  passing  into  brown,  and  the  most  distant  of  a  bluish 
white  color.  If  this  incrustation  be  heated  under  the  reducing 
flame,  it  disappears  with  a  blue  flame. 

Metallic  iodides  and  bromides  behave  upon  charcoal  in  a 
similar  manner  to  the  chlorides.  Those  principally  deserving 
of  mention  are  the  bromides  and  iodides  of  potassium  and 
sodium.  These  fuse  upon  charcoal,  are  absorbed  into  its  pores, 
and  volatilize  in  the  form  of  white  fumes,  which  are  deposited 
upon  the  charcoal  at  some  distance  from  the  assay.  When 
the  saline  films  so  formed  are  submitted  to  the  reducing  flame, 
they  disappear,  coloring  the  flame  in  the  same  manner  as  the 
corresponding  chlorides. 

4.     EXAMINATIONS    IN    THE    PLATINUM    FORCEPS. 

Before  the  student  attempts  to  make  an  examination  in  the 
platinum  forceps  or  tongs,  he  should  first  ascertain  whether 


62  THE    BLOWPIPE. 

or  not  it  will  act  upon  the  platinum.  If  the  substance  to  be 
examined  shall  act  chemically  upon  the  platinum,  then  it 
should  be  examined  on  the  charcoal,  and  the  color  of  the 
flame  ascertained  as  rigidly  as  possible.  The  following  list  of 
substances  produce  the  color  attached  to  them. 


A.      VIOLET. 


Potash,  and  all  its  compounds,  with  the  exception  of  the  phosphate 
and  the  borate,  tinge  the  color  of  the  flame  violet. 


Chloride  of  copper, ...  .Intense  blue. 

Lead, Pale  clear  blue. 

Bromide  of  copper, Bluish  green. 

Antimony, Bluish  green. 

Selenium, Blue. 

Arsenic, English  green. 

C.       GKEEN. 

Ammonia,  Dark  green. 

Boracic  acid, Dark  green. 

Copper, Dark  green. 

Tellurium, Dark  green. 

Zinc, Light  green. 

Baryta. . Apple  green. 

Phosphoric  acid, Pale  green. 

Molybdic  acid, Apple  green. 

Telluric  acid, Light  green. 

D.     YELLOW. 

Soda, Intense  yellow. 

Water, Fe.eble  yellow. 

E.       RED. 

Strontia, Intense  crimson. 

Lithia,    Purplish  red. 

Potash, Violet  red. 

Lime, Purplish  red. 


INITIATORY     ANALYSIS.  63 

The  student  may  often  be  deceived  in  regard  to  the  colors  : 
for  instance,  if  a  small  splinter  of  almost  any  mineral  be  held 
at  the  point  of  the  flame  of  oxidation,  it  will  impart  a  very  slight 
yellow  to  the  flame.  This  is  caused,  doubtless,  by  the  water 
contained  in  the  mineral.  If  the  piece  of  platinum  wire  is  used, 
and  it  should  be  wet  with  the  saliva,  as  is  frequently  done  by 
the  student,  then  the  small  quantity  of  soda  existing  in  that 
fluid  will  color  the  flame  of  a  light  yellow  hue. 

A.       THE    VIOLET    COLOR. 

The  salts  of  potash,  with  the  exception  of  the  borate  and 
the  phosphate,  color  the  flame  of  a  rich  violet  hue.  This  color 
is  best  discovered  in  the  outer  flame  of  the  blowpipe,  as  is  the 
case  with  all  the  other  colors.  The  flame  should  be  a  small 
one,  with  a  lamp  having  a  small  wick,  while  the  orifice  of  the 
blowpipe  must  be  quite  small.  These  experiments  should  like 
wise  be  made  in  a  dark  room,  so  that  the  colors  may  be 
discerned  with  the  greatest  ease.  In  investigating  with 
potash  for  the  discernment  of  color,  it  should  be  borne  in  mind 
that  the  least  quantity  of  soda  will  entirely  destroy  the  violet 
color  of  the  potash,  by  the  substitution  of  its  own  strong 
yellow  color.  If  there  be  not  more  than  the  two  hundredth 
part  of  soda,  the  violet  reaction  of  the  potash  will  be  destroyed. 
This  is  likewise  the  case  with  the  presence  of  lithia,  for  its 
peculiar  red  color  will  destroy  the  violet  of  the  potash.  There 
fore  in  making  investigations  with  the  silicates  which  contain 
potash,  the  violet  color  of  the  latter  can  only  be  discerned 
when  they  are  free  from  soda  and  lithia. 

B.       THE    BLUE    COLOR. 

(a.)  The  Chloride  of  Copper. — Any  of  the  chlorides  produce 
a  blue  color  in  the  blowpipe  flame,  or  any  salt  which  contains 
chlorine  will  show  the  blue  tint,  as  the  color  in  this  case  is 
referable  to  the  chlorine  itself.  There  are,  however,  some 


64  T  H  E      B  L  O  W  P  I  P  E  . 

chlorides  which,  in  consequence  of  the  peculiar  reactions  of 
their  bases,  will  not  produce  the  blue  color,  although  in  these 
cases  the  blue  of  the  chlorine  will  be  very  likely  to  blend  itself 
with  the  color  produced  by  the  base.  The  chloride  of  copper 
communicates  an  intense  blue  to  the  flame,  when  fused  on  the 
platinum  wire.  If  the  heat  be  continued  until  the  chlorine 
is  driven  off,  then  the  greenish  hue  of  the  oxide  of  copper  will 
be  discerned. 

(b.)  Lead. — Metallic  lead  communicates  to  the  flame  a  pale 
blue  color.  The  oxide  reacts  in  the  same  manner.  The  lead- 
salts,  whose  acids  do  not  interfere  with  the  color,  impart  also 
a  fine  blue  to  the  flame,  either  in  the  platina  forceps,  or  the 
crooked  wire. 

(c.)  Bromide  of  Copper. — This  salt  colors  the  flame  of  a 
bluish-green  color,  but  when  the  bromine  is  driven  off,  then  we 
have  the  green  of  the  oxide  of  copper. 

(d.)  Antimony. — This  metal  imparts  a  blue  color  to  the 
blowpipe  flame,  but  if  the  metal  is  in  too  small  a  quantity, 
then  the  color  is  a  brilliant  white.  If  antimony  is  fused  on 
charcoal,  the  fused  metal  gives  a  blue  color.  The  white  subli 
mate  which  surrounds  the  fused  metal,  being  subjected  to  the 
flame  of  oxidation,  disappears  from  the  charcoal  with  a 
bluish-green  color. 

(e.)  Selenium. — If  fused  in  the  flame  of  oxidation,  it  imparts 
to  the  flame  a  deep  blue  color.  The  incrustation  upon  char 
coal  gives  to  the  flame  the  same  rich  color. 

(/,)  Arsenic. — The  arseniates  and  metallic  arsenic  itself 
impart  to  the  blowpipe  flame  a  fine  blue  color,  provided  that 
there  is  no  other  body  present  which  may  have  a  tendency  to 
color  the  flame  with  its  characteristic  hue.  The  sublimate  of 
arsenious  acid  which  surrounds  the  assay,  will  give  the  same 
blue  flame,  when  dissipated  by  the  oxidation  flame.  The 
platinum  forceps  will  answer  for  the  exhibition  of  the  color  of 
arsenic,  even  though  the  salts  be  arseniates,  whose  bases  possess 
the  property  of  imparting  their  peculiar  color  to  the  flame, 
such  as  the  arseniate  of  lime 


INITIATORY     ANALYSIS.  65 


C.       THE    GREEN    COLOR. 

(a.)  Ammonia. — The  salts  of  ammonia,  when  heated  before 
the  blowpipe,  and  just  upon  the  point  of  disappearing,  impart 
to  the  flame  a  feeble  though  dark  green  color.  This  color, 
however,  can  only  be  discerned  in  a  dark  room. 

(b.)  Boradc  Add. — If  any  one  of  the  borates  is  mixed  with 
two  parts  of  a  flux  composed  of  one  part  of  pulverized  fluor 
spar,  and  four  and  a  half  parts  of  bisulphate  of  potash,  and 
after  being  melted,  is  put  upon  the  coil  of  a  platinum  wire, 
and  held  at  the  point  of  the  blue  flame,  soon  after  fusion  takes 
place  a  dark  green  color  is  discerned,  but  it  is  not  of  long 
duration.  The  above  process  is  that  recommended  by  Dr. 
Turner.  The  green  color  of  the  borates  may  be  readily  seen 
by  dipping  them,  previously  moistened  with  sulphuric  acid, 
into  the  upper  part  of  the  blue  flame,  when  the  color  can 
be  readily  discerned.  If  soda  be  present,  then  the  rich  green 
of  the  boracic  acid  is  marred  by  the  yellow  of  the  soda.  Borax, 
or  the  biborate  of  soda  (NaO,  2BOs)  may  be  used  for  this 
latter  reaction,  but  if  it  be  moistened  with  sulphuric  acid,  the 
green  of  the  boracic  acid  can  then  be  seen.  If  the  borates, 
or  minerals  which  contain  boracic  acid,  are  fused  on  charcoal 
with  carbonate  of  potash,  then  moistened  with  sulphuric  acid 
and  alcohol,  then  the  bright  green  of  the  boracic  acid  is  pro 
duced,  even  if  the  mineral  contains  but  a  minute  portion  of 
the  boracic  acid. 

(c.)  Copper.  Nearly  all  the  ores  of  copper  and  its  salts, 
give  a  bright  green  color  to  the  blowpipe  flame.  Metallic 
copper  likewise  colors  the  flame  green,  being  first  oxidized. 
If  iodine,  chlorine,  and  bromine  are  present,  the  flame  is  con 
siderably  modified,  but  the  former  at  least  intensifies  the  color. 
Many  ores  containing  copper  also  color  the  flame  green,  but 
the  internal  portion  is  of  a  bright  blue  color  if  the  compound 
contains  lead,  the  latter  color  being  due  to  the  lead.  The 
native  sulphide  and  carbonate  of  copper  should  be  moistened 


66  THE    BLOWPIPE. 

with  sulphuric  acid,  while  the  former  should  be  previously 
roasted.  If  hydrochloric  acid  is  used  for  moistening  the  salts, 
then  the  rich  green  given  by  that  moistened  with  the  sulphuric 
acid  is  changed  to  a  blue,  being  thus  modified  by  the  chlorine 
of  the  acid.  Silicates  containing  copper,  if  heated  in  the  flame 
in  the  platinum  forceps,  impart  a  rich  green  color  to  the  outer 
flame.  In  fact,  if  any  substance  containing  copper  be  sub 
mitted  to  the  blowpipe  flame,  it  will  tinge  it  green,  provided 
there  be  no  other  substance  present  to  impart  its  own  color 
to  the  flame,  and  thus  modify  or  mar  that  of  the  copper. 

(d.)  Tellurium. — If  the  flame  of  reduction  is  directed  upon 
the  oxide  of  tellurium  placed  upon  charcoal,  a  green  color  is 
imparted  to  it.  If  the  telluric  acid  be  placed  upon  platinum 
wire  in  the  reduction  flame,  the  oxidation  flame  is  colored 
green.  Or  if  the  sublimate  be  dissipated  by  the  flame  of 
oxidation,  it  gives  a  green  color.  If  selenium  be  present,  the 
green  color  is  changed  to  a  blue. 

(e.)  Zinc. — The  oxide  of  zinc,  when  strongly  heated,  gives  a 
blue  flame.  This  is  especially  the  case  in  the  reducing  flame. 
The  flame  is  a  small  one,  however,  and  not  very  characteristic, 
as  with  certain  preparations  of  zinc  the  blue  color  is  changed 
to  a  bright  white.  The  soluble  salts  of  zinc  give  no  blue  color. 

(/.)  Baryta. — The  soluble  salts  of  baryta,  moistened,  and 
then  submitted  to  the  reduction  flame,  produce  a  green  color. 
The  salt  should  be  moistened,  when  the  color  will  be  strongly 
marked  in  the  outer  flame.  The  insoluble  salts  do  not  produce 
so  vivid  a  color  as  the  soluble  salts,  and  they  are  brighter  when 
they  have  previously  been  moistened.  The  carbonate  does 
not  give  a  strong  color,  but  the  acetate  does,  so  long  as  it  is  not 
allowed  to  turn  to  a  carbonate.  The  chloride,  when  fused  on 
the  platinum  wire,  in  the  point  of  the  reduction  flame,  imparts 
a  fine  green  color  to  the  oxidation  flame.  This  tint  changes 
finally  to  a  faint  dirty  green  color.  The  sulphate  of  baryta 
colors  the  flame  green  when  heated  at  the  point  of  the  reduc 
tion  flame.  But  neither  the  sulphate,  carbonate,  nor,  in  fact, 
any  other  salt  of  baryta,  gives  such  a  fine  green  color  as  the 


INITIATORY     ANALYSIS.  67 

chloride.     The  presence  of  lime  does  interfere  with  the  reac 
tion  of  baryta,  but  still  does  not  destroy  its  color. 

(g.)  Phosphoric  Acid. — The  phosphates  give  a  green  color 
to  the  oxidation  flame,  especially  when  they  are  moistened 
with  sulphuric  acid.  This  is  best  shown  with  the  platinum 
forceps.  The  green  of  phosphoric,  or  the  phosphates,  is  much 
less  intense  than  that  of  the  borates  or  boracic  acid,  but  yet  the 
reaction  is  a  certain  one,  and  is  susceptible  of  considerable 
delicacy,  either  with  the  forceps,  or  still  better  upon  platinum 
wire.  Sulphuric  acid  is  a  great  aid  to  the  development 
of  the  color,  especially  if  other  salts  be  present  which  would 
be  liable  to  hide  the  color  of  the  phosphoric  acid.  In  this 
reaction  with  phosphates,  the  water  should  be  expelled  from 
them  previous  to  melting  them  with  sulphuric  acid.  They 
should  likewise  be  pulverized.  Should  soda  be  present  it  will 
only  exhibit  its  peculiar  color  after  the  phosphoric  acid  shall 
have  been  expelled  ;  therefore,  the  green  color  of  the  phos 
phoric  acid  should  be  looked  for  immediately  upon  submitting 
the  phosphate  to  heat. 

(h.)  Molybdic  Acid. — If  this  acid  or  the  oxide  of  molybde 
num  be  exposed  upon  a  platinum  wire  to  the  point  of  the 
reduction  flame,  a  bright  green  color  is  communicated  to  the 
flame  of  oxidation.  Take  a  small  piece  of  the  native  sulphide 
of  molybdenum,  and  expose  it  in  the  platinum  tongs  to  the 
flame  referred  to  above,  when  the  green  color  characteristic  of 
this  metal  will  be  exhibited. 

(i.)  Telluric  Acid. — If  the  flame  of  reduction  is  directed 
upon  a  small  piece  of  the  oxide  of  tellurium  placed  upon  char 
coal,  a  bright  green  color  is  produced.  Or  if  telluric  acid  be 
submitted  to  the  reduction  flame  upon  the  loop  of  a  platinum 
wire,  it  communicates  to  the  outer  flame  the  bright  green  of 
tellurium.  If  the  sublimate  found  upon  the  charcoal  in  the 
first  experiment  be  submitted  to  the  blowpipe  flame,  the  green 
color  of  tellurium  is  produced  while  the  sublimate  is  volatilized. 
If  selenium  be  present  the  green  color  is  changed  to  a  deep 
blue  one. 


68  THE    BLOW  PIPE. 


D.       YELLOW. 

- 

The  salts  of  soda  all  give  a  bright  yellow  color  when  heated 
in  the  platinum  loop  in  the  reduction  flame.  This  color  is 
very  persistent,  and  will  destroy  the  color  of  almost  any  other 
substance.  Every  mineral  of  which  soda  is  a  constituent, 
give  this  bright  orange-yellow  reaction.  Even  the  silicate  of 
soda  itself  imparts  to  the  flame  of  oxidation  the  characteristic 
yellow  of  soda. 

E.     RED. 

(a.)  Strontia. — Moisten  a  small  piece  of  the  chloride  of 
strontium,  put  it  in  the  platinum  forceps  and  submit  it  to  the 
flame  of  reduction,  when  the  outer  flame  will  become  colored 
of  an  intense  red.  If  the  salt  of  strontia  should  be  a  soluble 
one,  the  reaction  is  of  a  deeper  color  than  if  an  insoluble  salt 
is  used,  while  the  color  is  of  a  deeper  crimson  if  the  salt  is 
moistened.  If  the  salt  be  a  soluble  one,  it  should  be  moistened 
and  dipped  into  the  flame,  while  if  it  be  an  insoluble  salt,  it 
should  be  kept  dry  and  exposed  beyond  the  point  of  the  flame. 
The  carbonate  of  strontia  should  be  moistened  with  hydro 
chloric  acid  instead  of  water,  by  which  its  color  similates  that 
of  the  chloride  of  strontium  when  moistened  with  water.  In 
consequence  of  the  decided  red  color  which  strontia  commu 
nicates  to  flame,  it  is  used  by  pyrotechnists  for  the  purpose  of 
making  their  "  crimson  fire." 

(b.)  Lithia. — The  color  of  the  flame  of  lithia  is  slightly 
inclined  to  purple.  The  chloride,  when  placed  in  the  platinum 
loop,  gives  to  the  outer  flame  a  bright  red  color,  sometimes 
with  a  slight  tinge  of  purple.  Potash  does  not  prevent  this 
reaction,  although  it  may  modify  it  to  violet ;  but  the  decided 
color  of  soda  changes  the  red  of  lithia  to  an  orange  color.  If 
much  soda  be  present,  the  color  of  the  lithia  is  lost  entirely. 
The  color  of  the  chloride  of  lithium  may  be  distinctly  produced 
before  the  point  of  the  blue  flame,  and  its  durability  may  be 


INITIATORY     ANALYSIS.  69 

the  means  of  determining  it  from  that  of  lithium,  as  the  latter, 
under  the  same  conditions,  is  quite  evanescent.  The  minerals 
which  contain  lithia,  frequently  contain  soda,  and  thus  the  lat 
ter  destroys  the  color  of  the  former. 

(c.)  Potash. — The  salts  of  potash,  if  the  acid  does  not  inter 
fere,  give  a  purplish-red  color  before  the  blowpipe  ;  but  as  the 
color  is  more  discernibly  a  purple,  we  have  classed  it  under  that 
color. 

(d.)  Lime. — The  color  of  the  flame  of  lime  does  not  greatly 
differ  from  that  of  strontia,  with  the  exception  that  it  is  not  so 
decided.  Arragonite  and  calcareous  spar,  moistened  with  hydro 
chloric  acid,  and  tried  as  directed  for  strontia,  produce  a  red 
light,  not  unlike  that  of  strontia.  The  chloride  of  calcium  gives 
a  red  tinge,  but  not  nearly  so  decided  as  the  chloride  of  strontium. 
The  carbonate  of  lime  will  produce  a  yellowish  flame  for  a  while, 
until  the  carbonic  acid  is  driven  off,  when  the  red  color  of  the 
lime  may  be  discerned. 

If  the  borate  or  phosphate  of  lime  be  used,  the  green  color 
of  the  acids  predominates  over  the  red  of  the  lime.  Baryta  also 
destroys  the  red  color  of  the  lime,  by  mixing  its  green  color 
with  it.  There  is  but  one  silicate  of  lime  which  colors  the 
flame  red,  it  is  the  variety  termed  tabular  spar. 

5.    EXAMINATIONS    IN   THE    BORAX    BEAD. 

In  order  to  examine  a  substance  in  borax,  the  loop  of  the 
platinum  wire  should,  after  being  thoroughly  cleaned,  and 
heated  to  redness,  be  quickly  dipped  into  the  powdered 
borax,  and  then  quickly  transferred  to  the  flame  of  oxidation, 
and  there  fused.  If  the  bead  is  not  large  enough  to  fill  the 
loop  of  the  wire,  it  must  be  subjected  again  to  the  same  pro 
cess.  By  examining  the  bead,  both  when  hot  and  cold,  by 
holding  it  up  against  the  light,  it  can  be  soon  ascertained  whe 
ther  it  is  free  from  dirt  by  the  transparency,  or  the  want  of  it,  of 
the  bead. 

In  order  to  make  the  examination  of  a  substance,  the  bead 


TO  THE     BLOWPIPE. 

should  be  melted  and  pressed  against  it,  when  enough  will 
adhere  to  answer  the  purpose.  This  powder  should  then  be 
fused  in  the  oxidation  flame  until  it  mixes  with,  and  is  tho 
roughly  dissolved  by  the  borax  bead. 

The  principal  objects  to  be  determined  now  are  :  the  color  of 
the  borax  bead,  both  when  heated  and  when  cooled  ;  also  the 
rapidity  with  which  the  substance  dissolves  in  the  bead,  and  if 
•any  gas  is  eliminated. 

If  the  color  of  the  bead  is  the  object  desired,  the  quantity  of 
the  substance  employed  must  be  very  small,  else  the  bead  will 
be  so  deeply  colored,  as  in  some  cases  to  appear  almost  opaque, 
as,  for  instance,  in  that  of  cobalt.  Should  this  be  the  case, 
then,  while  the  bead  is  still  red  hot,  it  should  be  pressed  flat 
with  the  forceps  ;  or  it  may,  while  soft,  be  pulled  out  to  a  thin 
thread,  whereby  the  color  can  be  distinctly  discovered. 

Some  bodies,  when  heated  in  the  borax  bead,  present  a  clear 
bead  both  while  hot  and  cold  ;  but  if  the  bead  be  heated 
with  the  intermittent  flame,  or  in  the  flame  of  reduction,  it 
becomes  opalescent,  opaque  or  milk-white.  The  alkaline  earths 
are  instances  of  this  kind  of  reaction,  also  gluciua  oxide 
of  cerium,  tantalic  and  titanic  acids,  yttria  and  zircouia. 
But  if  a  small  portion  of  silica  should  be  present,  then  the  bead 
becomes  clear.  This  is  likewise  the  case  with  some  silicates, 
provided  there  be  not  too  large  a  quantity  present,  that  is  :  over 
the  quantity  necessary  to  saturate  the  borax,  for,  in  that  case, 
the  bead  will  be  opaque  when  cool. 

If  the  bead  be  heated  on  charcoal,  a  small  tube  or  cavity 
must  be  scooped  out  of  the  charcoal,  the  bead  placed  in  it,  and 
the  flame  of  reduction  played  upon  it.  When  the  bead  is  per 
fectly  fused,  it  is  taken  up  between  the  platinum  forceps  and 
pressed  flat,  so  that  the  color  may  be  the  more  readily  discerned. 
This  quick  cooling  also  prevents  the  protoxides,  if  there  be  any 
present,  from  passing  into  a  higher  degree  of  oxidation. 

The  bead  should  first  be  submitted  to  the  oxidation  flame, 
and  any  reaction  carefully  observed.  Then  the  bead  should  be 
submitted  to  the  flame  of  reduction.  It  must  be  observed  that 


INITIATORY     ANALYSIS.  71 

the  platinum  forceps  should  not  be  used  when  there  is  danger 
of  a  metallic  oxide  being  reduced,  as  in  this  case  the  metal 
would  alloy  with  the  platinum  and  spoil  the  forceps.  In  this 
case  charcoal  should  be  used  for  the  support.  If,  however, 
there  be  oxides  present  which  are  not  reduced  by  the  borax, 
then  the  platinum  loop  may  be  used.  Tin  is  frequently  used 
for  the  purpose  of  enabling  the  bead  to  acquire  a  color  for  an 
oxide  in  the  reducing  flame,  by  its  affinity  for  oxygen.  The 
oxide,  thus  being  reduced  to  a  lower  degree  of  oxidation, 
imparts  its  peculiar  tinge  to  the  bead  as  it  cools. 

The  arsenides  and  sulphides,  before  being  examined,  should 
be  roasted,  and  then  heated  with  the  borax  bead.  The  arsenic 
of  the  former,  it  should  be  observed,  will  act  on  the  glass  tube 
in  which  the  sublimation  is  proceeding,  if  the  glass  should 
contain  lead. 

It  should  be  recollected  that  earths,  metallic  oxides,  and 
metallic  acids  are  soluble  in  borax,  except  those  of  the  easily 
reducible  metals,  such  as  platinum  or  gold,  or  of  mercury,  which 
too  readily  vaporize.  Also  the  metallic  sulphides,  after  the 
sulphur  has  been  driven  off.  Also  the  salts  of  metals,  after 
their  acids  are  driven  off  by  heat.  Also  the  nitrates  and  car 
bonates,  after  their  acids  are  driven  off  during  the  fusion. 
Also  the  salts  of  the  halogens,  such  as  the  chlorides,  iodides, 
bromides,  etc.,  of  the  metals.  Also  the  silicates,  but  with 
great  tardiness.  Also  the  phosphates  and  borates  that  fuse  in 
the  bead  without  suffering  decomposition.  The  metallic  sul 
phides  are  insoluble  in  borax,  and  many  of  the  metals  in  the 
pure  state. 

There  are  many  substances  which  give  clear  beads  with 
borax  both  while  hot  and  cold,  but  which,  upon  being  heated 
with  the  intermittent  oxidation  flame,  become  enamelled  and 
opaque.  The  intermittent  flame  may  be  readily  attained, 
not  by  varying  the  force  of  the  air  from  the  mouth,  but  by 
raising  and  depressing  the  bead  before  the  point  of  the  steady 
oxidating  flame.  The  addition  of  a  little  nitrate  of  potash 
will  often  greatly  facilitate  the  production  of  a  color,  as  it 


72  THE    BLOWPIPE. 

oxidizes  the  metal.  The  hot  bead  should  be  pressed  upon  a 
small  crystal  of  the  nitrate,  when  the  bead  swells,  intumescesf 
and  the  color  is  manifested  in  the  surface  of  the  bead. 


6.      EXAMINATIONS    IN   MICROCOSMIC    SALT. 

Microcosmic  salt  is  a  better  flux  for  many  metallic  oxides 
than  borax,  as  the  colors  are  exhibited  in  it  with  more  strength 
and  character.  Microcosmic  salt  is  the  phosphate  of  soda  and 
ammonia.  When  it  is  ignited  it  passes  into  the  biphosphate 
of  soda,  the  ammonia  being  driven  off.  This  biphosphate  of 
soda  possesses  an  excess  of  phosphoric  acid,  and  thus  has 
the  property  of  dissolving  a  great  number  of  substances,  in 
fact  almost  any  one,  with  the  exception  of  silica.  If  the 
substances  treated  with  this  salt  consist  of  sulphides  or  arse 
nides,  the  bead  must  be  heated  on  charcoal.  But  if  the 
substance  experimented  upon  consists  of  earthly  ingredients 
or  metallic  oxides,  the  platinum  wire  is  the  best.  If  the  latter 
is  used  a  few  additional  turns  should  be  given  to  the  wire  in 
consequence  of  the  greater  fluidity  of  the  bead  over  that  of 
borax.  The  microcosmic  salt  bead  possesses  the  advantage 
over  that  of  borax,  that  the  colors  of  many  substances  are 
better  discerned  in  it,  and  that  it  separates  the  acids,  the  more 
volatile  ones  being  dissipated,  while  the  fixed  ones  combine 
with  a  portion  of  the  base  equally  with  the  phosphoric  acid, 
or  else  do  not  combine  at  all,  but  float  about  in  the  bead,  as 
is  the  case  particularly  with  silicic  acid.  Many  of  the 
silicates  give  with  borax  a  clear  bead,  while  they  form  with 
microcosmic  salt  an  opalescent  one. 

It  frequently  happens,  that  if  a  metallic  oxide  will  not  give 
its  peculiar  color  in  one  of  the  flames,  that  it  will  in  the  other, 
as  the  difference  in  degree  with  which  the  metal  is  oxidized 
often  determines  the  color.  If  the  bead  is  heated  in  the  re 
ducing  flame,  it  is  well  that  it  should  be  cooled  rapidly  to 
prevent  a  reoxidatiou.  Reduction  is  much  facilitated  by  the 
employment  of  metallic  tin,  whereby  the  protoxide  or  the 


INITIATORY     ANALPSIS.  73 

reduced   metal    may   be   obtained   in   a   comparatively   brief 
time. 

The  following  tables,  taken  from  Plattner  and  Sherer,  will 
present  the  reactions  of  the  metallic  oxides,  and  some  of  the 
metallic  acids,  in  such  a  clear'  light,  that  the  student  cannot 
very  easily  be  led  astray,  if  he  gives  the  least  attention  to  them. 
It  frequently  happens  that  a  tabular  statement  of  reactions 
will  impress  facts  upon  the  memory  when  long  detailed  descrip 
tions  will  fail  to  do  so.  It  is  for  this  purpose  that  we  subjoin 
the  following  excellent  tables. 


TABLE    I. 


A.    BORAX.  B.     MICROCOSMIC   SALT. 

1.  Oxydizing  flame.  1.  Oxydizing  flame. 

2.  Reducing       "  2.  Reducing       " 


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TABLE    II. 


87 


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93 


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99 


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'S  I' 


INITIATORY     ANALYSIS.  103 


t.       EXAMINATIONS    WITH    CARBONATE    OF    SODA. 

The  carbonate  of  soda  is  pulverized  and  then  kneaded  to  a 
paste  with  water;  the  substance  to  be  examined,  in  fine  powder, 
is  also  mixed  with  it.  A  small  portion  of  this  paste  is  placed 
on  the  charcoal,  and  gradually  heated  until  the  moisture  is 
expelled,  when  the  heat  is  brought  to  the  fusion  of  the  bead, 
or  as  high  as  it  can  be  raised.  Several  phenomena  will  take 
place,  which  must  be  closely  observed.  Notice  whether  the 
substance  fuses  with  the  bead,  and  if  so,  whether  there  is  intu 
mescence  or  not.  Or,  whether  the  substance  undergoes  reduc 
tion;  or,  whether  neither  of  these  reactions  takes  place,  and,  on 
the  contrary,  the  soda  sinks  into  the  charcoal,  leaving  the  sub 
stance  intact  upon  its  surface.  If  intumescence  takes  place,  the 
presence  of  either  tartaric  acid,  molybdic  acid,  silicic,  or  tung- 
stic  acid,  is  indicated.  The  silicic  acid  will  fuse  into  a  bead, 
which  becomes  clear  when  it  is  cold.  Titanic  acid  will  fuse 
into  the  bead,  but  may  be  easily  distinguished  from  the  silicic 
acid  by  the  bead  remaining  opaque  when  cold. 

Strontia  and  baryta  will  flow  into  the  charcoal,  but  lime  will 
not.  The  molybdic  and  tungstic  acids  combine  with  the  soda, 
forming  the  respective  salts.  These  salts  are  absorbed  by 
the  charcoal.  If  too  great  a  quantity  of  soda  is  used,  the  bead 
will  be  quite  likely  to  become  opaque  upon  cooling,  while,  if 
too  small  a  quantity  of  soda  is  used,  a  portion  of  the  substance 
will  remain  undissolved.  These  can  be  equally  avoided  by 
either  the  addition  of  soda,  or  the  substance  experimented 
upon,  as  may  be  required. 

As  silica  and  titanic  acid  are  the  only  two  substances  that 
produce  a  clear  bead,  the  student,  if  he  gets  a  clear  bead,  may 
almost  conclude  that  he  is  experimenting  with  silica,  titanic 
acid  being  a  rare  substance.  When  soda  is  heated  with 
silica,  a  slight  effervescence  will  be  the  first  phenomenon  no 
ticed.  This  is  the  escape  of  the  carbonic  acid  of  the  carbonate 
of  soda,  while  the  silicic  acid  takes  its  place,  forming  a  glass 


104  THE    BLOWPIPE. 

with  the  soda.  As  titanic  acid  will  not  act  in  the  same  man 
ner  as  silica,  it  can  be  easily  distinguished  by  its  bead  not 
being  perfectly  pellucid.  If  the  bead  with  which  silica  is 
fused  should  be  tinted  of  a  hyacinth  or  yellow  color,  this  may 
be  attributed  to  the  presence  of  a  small  quantity  of  sulphur  or 
a  sulphate,  and  this  sometimes  happens  from  the  fact  of  the 
flux  containing  sulphate  of  soda.  The  following  metals, 
when  exposed  with  carbonate  of  soda  to  the  reducing  flame, 
are  wholly  or  partially  reduced,  viz.  the  oxides  of  all  the 
noble  metals,  the  oxides  and  acids  of  tungsten,  molybdenum, 
arsenic,  antimony,  mercury,  copper,  tellurium,  zinc-,  lead,  bis. 
muth,  tin,  cadmium,  iron,  nickel,  and  cobalt.  Mercury  and 
arsenic,  as  soon  as  they  are  reduced,  are  dissipated,  while 
tellurium,  bismuth,  lead,  antimony,  cadmium,  and  zinc,  are  only 
partially  volatilized,  and,  therefore,  form  sublimates  on  the 
charcoal.  Those  metals  which  are  difficult  of  reduction  should 
be  fused  with  oxalate  of  potassa,  instead  of  the  carbonate  of 
soda.  The  carbonic  oxide  formed  from  the  combustion  of  the 
acid  of  this  salt  is  very  efficient  in  the  reduction  of  these  metals. 
Carbonate  of  soda  is  very  efficient  for  the  detection  of  minute 
quantities  of  manganese.  The  mixture  of  the  carbonate  of 
soda  with  a  small  addition  of  nitrate  of  potassa,  and  the 
mineral  containing  manganese,  must  be  fused  on  platinum 
foil.  The  fused  mass,  when  cooled,  presents  a  fine  blue  color. 

1.  The   following   minerals,    according   to    Griffin,    produce 
beads  with  soda,  but  do  not  fuse  when  heated  alone  :  quartz, 
agalmatolyte,    dioptase,    hisingerite,    sideroschilosite,    leucite, 
rutile,  pyrophyllite,  wolckonskoite. 

2.  The  following  minerals  produce   only  slags  with  soda  : 
allophane,  cymophane,  polymignite,  seschynite,  oerstedtite,  titaii- 
iferous  iron,  tantalite,  oxides  of  iron,  yttro-tantalite,  oxides  of 
manganese,  peroxide  of  tin  (is  reduced),  hydrate  of  alumina, 
hydrate  of  magnesia,  spinel,  gahnite,  worthite,   carbonate  of 
zinc,  pechuran,  zircon,  thorite,  andalusite,  staurolite,  gehlenite, 
chlorite  spar,  chrome  ochre,  uwarowite,  chromate  of  iron,  car 
bonates  of  the  earths,  carbonates  of  the  metallic  oxides,  basic 


INITIATO  R  Y     A  N  A  LYSIS.  105 

pho3phate  of  yttria,  do.  of  alamina.,  do.  of  lime,  persulphate  of 
iron,  sulphate  of  alumina,  aluminite,-  alumstone,  fluoride  of 
cerium,  yttrocerite,  topaz,  corundum,  pleonaste,  chondrodite. 

3.  The  following  minerals  produce  beads  with  a  small  quan 
tity  of  soda,  but  produce  slags  if  too  much  soda  is  added  : 
phenakite,  pierosmine,  olivine,  cerite,  cyanite,  talc,  gadolinite, 
lithium-tourmaline. 

1.  The  following  minerals,  when  fused  alone,  produce  beads. 
Of  these  minerals  the  following  produce  beads  with  soda  :  the 
zeolites,  spodumene,  soda-spodumene,  labrador,  scapolite,  socialite 
(Greenland),  elaeolite,  mica  from  primitive  lime-stone,   black 
talc,  acmite,  krokidolite,  lievrite,  cronstedtite,  garnet,  cerine, 
helvine,  gadolinite,  boracic  acid,  hydroboracite,  tincal,  boracite, 
datholite,  botryolite,  axinite,  lapis  lazuli,  eudialyte,  pyrosmalite, 
cryolite. 

2.  The  following  minerals  produce  beads  with  a  small  quan 
tity  of  soda,  but  if  too  much  is  added  they  produce  slags  : 
okenite,  pectolite,  red  silicate  of  manganese,  black  hydro-sili 
cate   of  manganese,   idocrase,   manganesian   garnets,   orthite, 
pyrorthite,  sordawalite,  sodalite,  fluorspar. 

3.  The  following  minerals  produce  a  slag  with  soda  :  brevi- 
cite,  amphodelite,  chlorite,  fahlunite,  pyrope,  soap-stone  (Cor 
nish)  red  dichroite,  pyrargillite,  black  potash  tourmaline,  wol 
fram,  pharmacolite,  scorodite,  arseniate  of  iron,  tetraphyline, 
hetepozite,  uranite,  phosphate  of  iron,  do.  of  strontia,  do.  of 
magnesia,  polyhalite,  hauyne. 

4.  The  following  metals  are  reduced  by  soda  :  tungstate  of 
lead,  molybdate  of  lead,  vanadate  of  lead,  chromate  of  lead, 
vauquelinite,  cobalt  bloom,  nickel  ochre,  phosphate  of  copper, 
sulphate  of  lead,  chloride  of  lead,  and  chloride  of  silver. 

The  following  minerals  fuse  on  the  edges  alone,  when  heated 
in  the  blow-pipe  flame  : 

1.  The  following  produce  beads  with  soda  :  steatite,  meer 
schaum,  felspar,  albite,  petalite,  nepheline,  anorthite,  emerald, 
euclase,  turquois,  sodalite  (Vesuvius), 

2.  The  following  minerals  produce  beads  with  a  small  quau- 


106  THE     BLOWPIPE. 

tity  of  soda,  but  with  the  addition  of  more  produce  slags  : 
tabular  spar,  diallage,  hypersthene,  epidote,  zoisite. 

3.  The  following  minerals  produce  slags  only  with  soda  : 
stilpnosiderite,  plombgomme,  serpentine,  silicate  of  manga 
nese  (from  Piedmont),  mica  from  granite,  pimelite,  pinite,  blue 
dichroite,  sphene,  karpholite,  pyrochlore,  tungstate  of  lime, 
green  soda  tourmaline,  lazulite,  heavy  spar,  gypsum. 

The  reactions  of  substances,  when  fused  with  soda  in  the 
flame  of  oxidation  may  be  of  use  to  the  student.  A  few  of 
them  are  therefore  given.  Silica  gives  a  clear  glass. 

The  oxid'e  of  tellurium  and  telluric  acid  gives  a  clear  bead 
when  it  is  hot,  but  white  after  it  is  cooled. 

Titanic  acid  gives  a  yellow  bead  when  hot. 

The  oxide  of  chromium  gives  also  a  clear  yellow  glass  when 
hot,  but  is  opaque  when  cold. 

Molybdic  acid  gives  a  clear  bead  when  hot,  but  is  turbid  and 
white  after  cooling. 

The  oxides  and  acids  of  antimony  give  a  clear  and  colorless 
bead  while  hot,  and  white  after  cooling. 

Vanadic  acid  is  absorbed  by  the  charcoal,  although  it  is  not 
reduced. 

Tungstic  acid  gives  a  dark  yellow  clear  bead  while  hot,  but 
is  opaque  and  yellow  when  cold. 

The  oxides  of  manganese  give  to  the  soda  bead  a  fine  char 
acteristic  green  color.  This  is  the  case  with  a  very  small  quan 
tity.  This  reaction  is  best  exhibited  on  platinum  foil. 

Oxide  of  cobalt  gives  to  the  bead  while  hot  a  red  color, 
which,  upon  being  cooled,  becomes  grey. 

The  oxide  of  copper  gives  a  clear  green  bead  while  hot. 

The  oxide  of  lead  gives  a  clear  colorless  bead  while  hot, 
which  becomes,  upon  cooling,  of  a  dirty  yellow  color  and 
opaque. 

The  following  metals,  when  they  are  fused  with  soda  on  char 
coal,  in  the  flame  of  reduction,  produce  volatile  oxides,  and 
leave  an  incrustation  around  the  assay,  viz.  bismuth,  zinc, 
lead,  cadmium,  antimony,  selenium,  tellurium,  and  arsenic. 


INITIATORY     ANALYSIS.  107 

Bismuth,  under  the  reduction  flame,  yields  small  particles  of 
metal,  which  are  brittle  and  easily  crushed.  The  incrustation 
is  of  a  flesh  color,  or  orange,  when  hot,  but  gets  lighter  as  it 
cools.  The  sublimate  may  be  driven  about,  the  charcoal  from 
place  to  place,  by  either  flame,  but  is  finally  dissipated.  While 
antimony  and  tellurium,  in  the  act  of  dissipation,  give  color  to 
the  flame,  bismuth  does  not,  and  may  thus  be  distinguished 
from  them. 

Zinc  deposits  an  incrustation  about  the  assay,  which  is  yel 
low  while  hot,  but  fades  to  white  when  cold.  The  reduction 
flame  dissipates  this  deposit,  but  not  that  of  oxidation.  All 
the  zinc  minerals  deposit  the  oxide  incrustation  about  the 
assay,  which,  when  moistened  with  a  solution  of  cobalt  and 
heated,  changes  to  green. 

Lead  is  very  easily  reduced,  in  small  particles,  and  may  be 
easily  distinguished  by  its  flattening  under  the  hammer,  unlike 
bismuth.  It  leaves  an  incrustation  around  the  assay  resem 
bling  that  of  bismuth,  in  the  color  of  it,  and  in  the  peculiar 
manner  in  which  it  lies  around  the  assay. 

Cadmium  deposits  a  dull  reddish  incrustation  around  the 
assay.  Either  of  the  flames  dissipate  the  sublimate  with  the 
greatest  readiness. 

Antimony  reduces  with  readiness.  At  the  same  time  it  yields 
considerable  vapor,  and  deposits  an  incrustation  around  the 
assay.  This  deposit  can  be  driven  about  on  the  charcoal  by 
either  of  the  flames.  The  flame  of  reduction,  however,  pro 
duces  the  light  blue  color  of  the  antimony. 

Selenium  is  deposited  on  the  charcoal  as  a  grey  metallic- 
looking  sublimate,  but  sometimes  appearing  purple  or  blue. 
If  the  reduction  flame  is  directed  on  this  deposit,  it  is  dissi 
pated  with  a  blue  light. 

Tellurium  is  deposited  on  the  charcoal  as  a  white  sublimate, 
sometimes  changing  at  the  margin  to  an  orange  or  red  color. 
The  oxidation  flame  drives  the  deposit  over  the  charcoal,  while 
the  reduction-flame  dissipates  it  with  a  greenish  color. 

Arsenic  is  vaporized  rapidly,  while  there  is  deposited  around 


108  THE     BLOWPIPE. 

the  assay  a  white  incrustation  of  arsenious  acid.  This  deposit 
will  extend  to  some  distance  from  the  assay,  and  is  readily  vol 
atilized,  the  reducing  flame  producing  the  characteristic  allia 
ceous  color. 

The  following  metals,  or  their  compounds,  are  reduced  when 
fused  with  soda  on  charcoal,  in  the  flame  of  reduction.  They 
are  reduced  to  metallic  particles,  but  give  no  incrustation,  viz. 
nickel,  cobalt,  iron,  tin,  copper,  gold,  silver,  platinum,  tungsten, 
and  molybdenum. 

The  particles  of  iron,  nickel,  and  cobalt,  it  should  be  borne 
in  mind,  are  attracted  by  the  magnet. 

The  following  substances  are  neither  fused  nor  reduced  in 
soda,  viz.  alumina,  magnesia,  lime,  baryta,  strontia,  the  oxide 
of  uranium,  the  oxides  of  cerium,  zirconia,  tantalic  acid,  tho- 
rina,  glucina,  and  yttria.  Neither  are  the  alkalies,  as  they 
sink  into  the  charcoal.  The  carbonates  of  the  earths,  strontia, 
and  baryta  fuse. 


Part     III. 


SPECIAL    REACTIONS  ;     OR,    THE    BEHAVIOR    OP 
SUBSTANCES   BEFORE   THE   BLOWPIPE. 

ANALYTICAL  CHEMISTRY  may  be  termed  the  art  of  converting 
the  unknown  constituents  of  substances,  by  means  of  certain 
operations,  into  new  combinations  which  we  recognize  through 
the  physical  and  chemical  properties  which  they  manifest. 

It  is,  therefore,  indispensably  necessary,  not  only  to  be  cogni 
zant  of  the  peculiar  conditions  by  which  these  operations  can 
be  effected,  but  it  is  absolutely  necessary  to  be  acquainted  with 
the  forms  and  combinations  of  the  resulting  product,  and  with 
every  modification  which  may  be  produced  by  altering  the  con 
ditions  of  the  analysis. 

We  shall  first  give  the  behavior  of  simple  substances  before 
the  blowpipe  ;  and  the  student  should  study  this  part  thor 
oughly,  by  repeating  each  reaction,  so  that  he  can  acquire  a 
knowledge  of  the  color,  form,  and  physical  properties  in  gene 
ral,  of  the  resulting  combination.  There  is  nothing,  perhaps, 
which  will  contribute  more  readily  to  the  progress  of  the  pupil, 
than  thorough  practice  with  the  reactions  recommended  in  this 
part  of  the  work,  for  when  once  the  student  shall  have  acquired 
a  practical  eye  in  the  discernment  of  the  peculiar  appearances 

109 


110  THE    BLOWPIPE. 

of  substances  after  they  have  undergone  the  decompositions 
produced  by  the  strong  heat  of  the  blowpipe  flame,  together 
with  the  reactions  incident  to  these  changes,  then  he  will  have 
greatly  progressed  in  his  study,  and  the  rest  will  be  compara 
tively  simple. 

A.     METALLIC   OXIDES. 

GROUP      FIRST. THE     ALKALIES:    POTASSA,      SODA,     AMMONIA,     AND 

LITHIA. 

The  alkalies,  in  their  pure,  or  carbonated  state,  render  red 
dened  litmus  paper  blue.  This  is  likewise  the  case  with  the 
sulphides  of  the  alkalies.  The  neutral  salts  of  the  alkalies, 
formed  with  the  strong  acids,  do  not  change  litmus  paper,  but 
the  salts  formed  with  the  weak  acids,  render  the  red  litmus  paper 
blue;  for  instance,  the  alkaline  salts  with  boracic  acid.  Fused 
with  borax,  soda,  or  microcosmic  salt,  they  give  a  clear  bead. 
The  alkalies  and  their  salts  melt  at  a  low  red  heat.  The  alka 
lies  cannot  be  reduced  to  the  metallic  state  before  the  blow 
pipe.  They  are  not  volatile  when  red  hot,  except  the  alkali 
ammonia,  but  they  are  volatile  at  a  white  heat. 

(a.)  Potassa  (KO). — It  is  not  found  free,  but  in  combina 
tion  with  inorganic  and  organic  acids,  as  well  in  the  animal  as 
in  the  vegetable  organism,  as  in  the  mineral  kingdom.  In  the 
pure,  or  anhydrous  state,  or  as  the  carbonate,  potassa  absorbs 
moisture,  and  becomes  fluid,  or  is  deliquescent,  as  it  is  termed. 
By  exposing  potassa,  or  its  easily  fusible  salts  (except  the  phos 
phate  or  borate),  upon  platinum  wire,  to  the  point  of  the  blue 
flame,  there  is  communicated  to  the  external  flame  a  violet 
color,  in  consequence  of  a  reduction  and  reoxidation.  This 
color,  though  characteristic"  of  all  the  potassa  compounds,  is 
scarcely  visible  with  the  phosphate  or  borate  salts  of  that 
alkali.  The  admixture  of  a  very  little  soda  (g-^th)  destroys 
the  color  imparted  by  the  potassa,  while  the  flame  assumes  a 
yellow  color,  characteristic  of  the  soda.  The  presence  of  lithia 
changes  the  violet  color  of  the  potash  into  red.  The  silicates 


SPECIAL     REACTIONS.  Ill 

of  potassa  must  exist  in  pretty  large  proportion  before  they  can 
be  detected  by  the  violet  color  of  the  flame,  and  those  minerals 
must  melt  easily  at  the  edges.  The  presence  of  a  little  soda  in 
these  instances  conceals  the  reaction  in  the  potassa  entirely. 

If  alcohol  is  poured  over  potassa  compounds  which  are  pow 
dered,  and  then  set  on  fire,  the  external  flame  appears  violet- 
colored,  particularly  when  stirred  with  a  glass  rod,  and  when 
the  alcohol  is  really  consumed.  The  presence  of  soda  in  lithia 
will,  in  this  case  likewise,  hide  by  their  own  characteristic 
color,  that  of  the  potassa. 

The  salts  of  potassa  are  absorbed  when  fused  upon  charcoal. 
The  sulphur,  bromine,  chlorine,  and  iodine  compounds  of  potassa 
give  a  white,  but  easily  volatile  sublimate  upon  the  charcoal, 
around  the  place  where  the  fused  substance  reposed.  This 
white  sublimate  manifests  itself  only  when  the  substance  is 
melted  and  absorbed  within  the  charcoal,  and  ceases  to  be 
visible  as  soon  as  it  is  submitted  to  the  reducing  flame,  while 
the  external  flame  is  colored  violet;  sulphate  of  potassa,  for 
instance,  is  reduced  by  the  glowing  charcoal  into  the  sulphide. 
This  latter  is  somewhat  volatile,  but  by  passing  through  the 
oxidation  flame,  it  is  again  oxidized  into  the  sulphate.  This, 
being  less  volatile,  sublimes  upon  the  charcoal,  but  by  expos 
ing  it  again  to  the  flame  of  reduction,  it  is  reduced  and  carried 
off  to  be  again  oxidized  by  its  passage  through  the  oxidation 
flame. 

Potassa  and  its  compounds  give,  with  soda,  borax  or  micro- 
cosmic  salt,  as  well  when  hot  as  cold,  colorless  beads,  unless 
the  acid  associated  with  the  alkali  should  itself  produce  a 
color.  When  borax  is  fused  with  some  pure  boracic  acid,  and 
sufficient  of  the  oxide  of  nickel  is  added,  so  that  the  beads 
appear  of  a  brown  color  after  being  cooled,  and  then  the  bead 
thus  produced  fused  with  the  substance  suspected  to  contain 
potassa,  in  the  oxidation  flame,  the  brown  color  is  changed 
to  blue.  The  presence  of  the  other  alkalies  does  not  prevent 
this  reaction.  As  it  is  not  possible  to  detect  potassa  com 
pound  with  unerring  certainty  by  the  blowpipe  flame,  the 


112  T  H   K        B  L  O   W  P  I  P   E. 

the  wet  method  should  be  resorted  to  for  the  purpose  of 
confirming  it. 

The  silicates  of  potassa  must  be  prepared  as  follows,  for  ana 
lytical  purposes  by  the  wet  way.  Mix  one  part  of  the  finely 
powdered  substance  with  two  parts  of  soda  (free  from  potassa), 
and  one  part  of  borax.  Fuse  the  mixture  upon  charcoal  in  the 
oxidation  flame  to  a  clear,  transparent  bead.  This  is  to  be 
exposed  again  with  the  pincers  to  the  oxidation  flame,  to  burn 
off  the  adhering  coal  particles.  Then  pulverize  and  dissolve  in 
hydrochloric  acid  to  separate  the  silica;  evaporate  to  dryness, 
dissolve  the  residue  in  water,  with  the  admixture  of  a  little 
alcohol,  and  test  the  filtrate  with  chloride  of  platinum  for  pot" 
assa. 

(&.)  Soda  (NaO). — This  is  one  of  the  most  abundant  sub. 
stances,  although  seldom  found  free,  but  combined  with  chlorine 
or  some  other  less  abundant  compound.  Soda,  its  hydrate  and 
salts  manifest  in  general  the  same  properties  as  their  respective 
potash  compounds  ;  but  the  salts  of  soda  mostly  contain  crystal 
water,  which  leaves  the  salts  if  they  are  exposed  to  the  air,  and 
the  salts  effervesce. 

By  exposing  soda  or  its  compounds  upon  a  platinum  wire  to 
the  blue  flame,  a  reddish-yellow  color  is  communicated  to  the 
external  flame,  which  appears  as  a  long  brilliant  stream  and 
considerably  increased  in  volume.  The  presence  of  potash  does 
not  prevent  this  reaction  of  soda.  If  there  is  too  large  a 
quantity  of  potash,  the  flame  near  to  the  substance  is  violet- 
colored,  but  the  edge  of  the  flame  exhibits  the  characteristic 
tint  of  the  soda.  The  presence  of  lithia  changes  the  yellow 
color  to  a  shade  of  red. 

When  alcohol  is  poured  over  powdered  soda  compounds  and 
lighted,  the  flame  exhibits  a  reddish-yellow  color,  particularly 
if  the  alcohol  is  stirred  up  with  a  glass  rod,  or  if  the  alcohol  is 
nearly  consumed. 

Fused  upon  charcoal,  soda  compounds  are  absorbed  by  the 
coal.  The  sulphide,  chloride,  iodide,  and  bromide  of  soda 
yield  a  white  sublimate  around  the  spot  where  the  substance  is 


SPECIAL     REACTIONS.  113 

laid,  but  this  sublimate  is  not  so  copious  as  that  of  the  potash 
compounds,  and  disappears  when  touched  with  the  reduction 
flame,  communicating  a  yellow  color  to  the  external  flame. 
The  presence  of  soda  in  compounds  must  likewise  be  confined 
bj  reactions  in  the  wet  way. 

(c.)  Ammonia  (NH40). — In  the  fused  state,  and  at  the 
usual  temperature,  ammonia  is  a  pungent  gas,  and  exerts  a 
reaction  upon  litmus  paper  similar  to  potash  and  soda. 
Ammonium  is  considered  by  chemists  as  a  metal,  from  the 
nature  of  its  behavior  with  other  substances.  It  has  not  beesi 
isolated,  but  its  existence  is  now  generally  conceded  by  all 
chemists.  The  ammonia  salts  are  volatile,  and  many  of  them 
sublimate  without  being  decomposed. 

The  salts  of  ammonia,  on  being  heated  in  the  point  of  the 
blue  flame,  produce  a  feeble  green  color  in  the  external  flame, 
just  previous  to  their  being  converted  into  vapor.  But  this 
color  is  scarcely  visible,  and  presents  nothing  characteristic. 
When  the  ammonia  salts  are  mixed  with  the  carbonate  of  soda, 
and  heated  in  a  glass  tube  closed  at  one  end,  carbonate  of 
ammonia  is  sublimed,  which  can  be  readily  recognized  by  its 
penetrating  smell  of  spirits  of  hartshorn. 

This  sublimate  will  render  blue  a  slip  of  red  litmus  paper. 
This  can  be  easily  done  by  moistening  the  litmus  paper,  and 
then  inserting  the  end  of  it  in  the  tube.  By  holding  a  glass 
rod,  moistened  with  dilute  hydrochloric  acid,  over  the  mouth 
of  the  tube,  a  white  vapor  is  instantly  rendered  visible  (sal 
ammoniac). 

(d.)  Lithia  (LiO). — In  the  pure  state,  lithia  is  white  and 
crystalline,  not  easily  soluble  in  water,  and  does  not  absorb 
moisture.  It  changes  red  litmus  to  blue,  and  at  a  low  red 
heat  it  melts.  Lithia  or  its  salts,  exposed  to  the  point  of  the 
blue  flame,  communicates  a  red  color  to  the  external  or 
oxidation  flame,  in  consequence  of  a  reduction,  sublimation, 
and  re-oxidation  of  the  lithia.  An  admixture  of  potash 
communicates  to  this  flame  a  reddish-violet  color,  and  the 
presence  of  soda  that  of  a  yellowish-red  or  orange.  If  the 


114:  THE     BLOWPIPE. 

soda,  however,  is  in  too  great  proportion,  then  its  intense 
yellow  hides  the  red  of  the  lithia.  In  the  latter  case  the  sub 
stance  under  test  must  be  only  imperfectly  fused  in  the  oxida 
tion  flame,  and  then  dipped  in  wax  or  tallow.  By  exposing  it 
now  to  the  reduction  flame,  the  red  color  imparted  to  the 
external  flame  by  the  lithia  becomes  visible,  even  if  a  consider 
able  quantity  of  soda  be  present.  A  particular  phenomenon 
appears  with  the  phosphate  of  lithia,  viz.,  the  phosphoric  acid 
itself  possesses  the  property  of  communicating  to  the  flame  a 
bluish-green  color.  By  its  combination  with  lithia  it  still 
exhibits  its  characteristic  color,  while  the  latter  presents  like 
wise  its  peculiar  tint.  Then  we  perceive  a  green  flame  in  the 
centre  of  the  flame,  while  the  red  color  of  lithia  surrounds  it. 

The  silicates,  which  contain  only  a  little  lithia,  produce  only 
a  slight  hue  in  the  flame,  and  often  none  at  all.  We  have  to 
mix  one  part  of  the  silicate  with  two  parts  of  a  mixture  com 
posed  of  one  part  of  fluorspar  and  one  and  a  half  parts  of  bi- 
sulphate  of  potassa.  Moisten  the  mass  with  water  so  that  the 
mass  will  adhere,  and  then  melt  it  upon  a  platinum  wire  in  the 
reduction  flame)  when  that  of  oxidation  will  present  the  red 
color  of  lithia. 

The  Borates  of  lithia  produce  at  first  a  green  color,  but 
it  soon  yields  to  the  red  of  lithia.  When  alcohol  is  poured 
over  lithia  or  its  compounds,  and  inflamed,  it  burns  with  a  deep 
red  color,  particularly  if  the  fluid  is  stirred  up  with  a  glass  rod, 
or  when  the  alcohol  is  nearly  consumed.  This  color  presents 
the  same  modifications  as  the  corresponding  ones  communicated 
to  the  blowpipe  as  mentioned  above. 

The  salts  of  lithia  are  absorbed  by  charcoal  when  fused  upon 
it.  The  sulphide,  bromide,  iodide,  and  chloride  of  lithia  pro 
duce  upon  the  charcoal  a  greyish-white  sublimate,  although 
not  so  copiously  as  the  corresponding  compounds  of  potash  and 
soda.  This  sublimate  disappears  when  touched  by  the  reduc 
tion  flame,  while  the  oxidation  flanie  gives  the  characteristic 
color  of  lithia, 


SPECIAL     REACTIONS.  115 


SECOND    GROUP. THE    ALKALINE    EARTHS,  BARYTA,    STROXTIA,  LIME, 

AND    MAGNESIA. 

Iii  the  pure  state,  the  alkaline  earths  are  caustic,  cause  red 
litmus  paper  to  become  blue,  and  are  more  or  less  soluble  in 
water.  Their  sulphides  are  also  soluble.  The  carbonates  and 
phosphates  of  the  alkaline  earths  are  insoluble  in  water.  By 
igniting  the  carbonates,  their  carbonic  acid  is  expelled,  and  the 
alkaline  earths  are  left  in  the  caustic  state.  The  alkaline  earths 
are  not  volatile,  and  their  organic  salts  are  converted,  by  igni 
tion,  into  carbonates. 

(a.)  Baryta.  (BaO). — This  alkaline  earth  does  not  occur 
free  in  nature,  but  combined  with  acids,  particularly  with  car 
bonic  and  sulphuric  acids.  In  the  pure  state,  baryta  is  of 
a  greyish-white  color,  presents  an  earthy  appearance,  and  is 
easily  powdered.  When  sparingly  moistened  with  water,  it 
slakes,  becomes  heated,  and  forms  a  dry,  white  powder.  With 
still  more  water  it  forms  a  crystalline  mass,  the  hydrate  of 
baryta,  which  is  completely  soluble  in  hot  water.  Pure 
baryta  is  infusible  ;  the  hydrate  fuses  at  a  red  heat,  without 
the  loss  of  its  hydratic  water;  if  caustic  baryta  is  exposed  for 
too  great  a  length  of  time  to  the  flame,  it  absorbs  water,  origi 
nated  by  the  combustion,  and  becomes  a  hydrate,  when  it  will 
melt.  Salts  of  baryta,  formed  with  most  acids,  are  insoluble 
in  water  ;  for  instance,  the  salts  with  sulphuric,  carbonic, 
arsenic,  phosphoric,  and  boracic  acids.  The  salts  of  baryta, 
soluble  in  water,  are  decomposed  by  ignition,  except  the  chlor 
ide. 

Carbonate  of  baryta  loses  its  carfionic  acid  at  a  red  heat, 
becomes  caustic,  and  colors  red  litmus  paper  blue. 

By  exposing  baryta  or  its  compounds  upon  a  platinum  wire, 
or  a  splinter  of  the  substance  held  with  the  platinum  tongs,  to 
the  point  of  the  blue  flame,  a  pale  apple-green  color  is  commu 
nicated  to  the  external  flame.  This  color  appears  at  first  very 
pale,  but  soon  becomes  more  intense.  This  color  is  most  visible 


116  THE     BLOWPIPE. 

if  the  substance  is  operated  with  in  small  quantities.  The 
chloride  of  barium  produces  the  deepest  color.  This  color  is 
less  intense  if  the  carbonate  or  sulphate  is  used.  The  presence 
of  strontia,  lime,  or  magnesia,  does  not  suppress  the  reaction  of 
the  baryta,  unless  they  greatly  predominate. 

When  alcohol  is  poured  over  baryta  or  its  salts,  and  inflamed, 
a  feeble  green  color  is  communicated  to  the  flame,  but  this 
color  should  not  be  considered  a  characteristic  of  the  salt. 

Baryta  and  its  compounds  give,  when  fused  with  carbonate 
of  soda  upon  platinum  foil,  a  clear  bead.  Fused  with  soda 
upon  charcoal,  it  is  absorbed.  The  sulphate  fuses  at  first  to  a 
clear  bead,  which  soon  spreads,  and  is  absorbed  and  converted 
while  boiling  into  a  hepatic  mass.  If  this  mass  is  taken  out, 
placed  upon  a  piece  of  polished  silver  and  moistened  with  a 
little  water,  a  black  spot  of  sulphide  of  silver  is  left  after  wash 
ing  off  the  mass  with  water. 

Borax  dissolves  baryta  and  its  compounds  with  a  hissing 
noise,  as  well  in  the  flame  of  oxidation  as  in  that  of  reduction. 
There  is  formed  a  clear  bead  which,  with  a  certain  degree  of 
saturation,  is  clear  when  cold,  but  appears  milk-white  when 
overcharged,  and  of  an  opal,  enamel  appearance,  when  heated 
intermittingiy,  or  with  a  vacillating  flame,  that  changes  fre 
quently  from  the  oxidating  to  the  reducing  flame.  Baryta  and 
its  compounds  produce  the  same  reactions  with  microcosmic  salt 

Baryta  and  its  compounds  fuse  when  exposed  to  ignition  in 
the  oxidizing  flame.  Moistened  with  the  solution  of  nitrate  of 
cobalt,  and  heated  in  the  oxidation  flame,  it  presents  a  bead, 
colored  from  brick-red  to  brown,  according  to  the  quantity 
used.  This  color  disappears  when  cold,  and  the  bead  falls  to  a 
pale  grey  powder  after  being  exposed  awhile  to  the  air.  When 
heated  again,  the  color  does  not  appear  until  fusion  is  effected. 
If  carbonate  of  soda  is  fused  upon  platinum  wire  with  so  much 
of  the  sesquioxide  of  manganese  that  a  green  bead  is  produced, 
this  bead,  when  fused  with  a  sufficient  quantity  of  baryta,  or 
its  compounds,  after  cooling;,  will  appear  of  a  bluish-green,  or 
light  blue  color. 


SPECIAL     REACTIONS.  117 

(&.)  Strontia  (SrO). — Strontia  and  its  compounds  are  ana 
logous  to  the  respective  ones  of  baryta.  The  hydrate  of 
strontia  has  the  same  properties  as  the  hydrate  of  baryta, 
except  that  it  is  less  soluble  in  water.  The  carbonate  of 
strontia  fuses  a  little  at  a  red  heat,  swells,  and  bubbles  up  like 
cauliflower.  This  produces,  in  the  blowpipe  flame,  an  intense 
and  splendid  light,  and  now  produces  an  alkaline  reaction  upon 
red  litmus  paper.  The  sulphate  of  strontia  melts  in  the  oxida- 
dation  flame  upon  platinum  foil,  or  upon^charcoal,  to  a  milk- 
white  globule.  This  fuses  upon  charcoal,  spreads  and  is 
reduced  to  the  sulphide,  which  is  absorbed  by  the  charcoal. 
It  now  produces  the  same  reactions  upon  polished  silver  as  the 
sulphate  of  baryta  under  the  same  conditions.  By  exposing 
strontia  and  its  compounds  upon  platinum  wire,  or  as  a  splinter 
with  the  platinum  tongs,  to  the  point  of  the  blue  flame,  the 
external  flame  appears  of  an  intense  crimson  color.  The  deep 
est  red  color  is  produced  by  the  chloride  of  strontium,  particu 
larly  at  the  first  moment  of  applying  the  heat.  After  the  salt 
is  fused,  the  red  color  ceases  to  be  visible  in  the  flame,  by 
which  it  is  distinguished  from  the  chloride  of  lithium.  The  car 
bonate  of  strontia  swells  up  and  produces  a  splendid  white 
light,  while  the  external  flame  is  colored  of  a  fine  purple-red. 
The  color  produced  by  the  sulphate  of  strontia  is  less  intense. 
The  presence  of  baryta  destroys  the  reaction  of  the  strontia, 
the  flame  presenting  the  light  green  color  oftthe  baryta. 

If  alcohol  is  poured  over  powdered  strontia  and  inflamed, 
the  flame  appears  purple  or  deep  crimson,  particularly  if  the 
fluid  is  stirred  with  a  glass  rod,  and  when  the  alcohol  is  nearly 
consumed. 

The  insoluble  salts  of  strontia  do  not  produce  a  very  intense 
color.  Baryta  does  not  prevent  the  reaction  of  the  soluble 
salts  of  strontia,  unless  it  exists  greatly  in  excess.  In  the 
presence  of  baryta,  strontia  can  be  detected  by  the  following 
process  :  mix  some  of  the  substance  under  examination  with 
some  pure  graphite  and  water,  by  grinding  in  an  agate  mortar. 
Place  the  mixture  upon  charcoal,  and  expose  it  for  a  while  to 


118  THE     BLOWPIPE. 

the  reduction  flame.  The  substance  becomes  reduced  to  sul 
phide  of  barium  and  sulphide  of  strontium,  when  it  should  be 
dissolved  in  hydrochloric  acid.  The  solution  should  be  evapo 
rated  to  dryness,  redissolved  in  a  little  water,  and  enough  alco 
hol  added  that  a  spirit  of  80  per  cent,  is  produced.  Inflame 
the  spirit,  and  if  strontia  is  present,  the  flame  is  tinged  of  a 
red  color.  This  color  can  be  discerned  more  distinctly  by 
moistening  some  cotton  with  this  spirit  and  inflaming  it. 

If  strontia  or  its  compounds  are  fused  with  a  green  bead  of 
carbonate  of  soda  and  sesquioxide  of  manganese,  as  described 
under  the  head  of  baryta,  a  bead  of  a  brown,  brownish-green, 
or  dark  grey  color  is  produced.  Carbonate  of  soda  does  not 
dissolve  pure  strontia.  The  carbonate  and  sulphate  of  strontia 
melt  with  soda  upon  platinum  foil  to  a  bead,  which  is  milk- 
white  when  cold,  but  fused  upon  charcoal  they  are  absorbed. 
Strontia  or  its  compounds  produce  with  borax,  or  microcosmic 
salt,  the  same  reactions  as  baryta.  When  they  are  moistened 
with  nitrate  of  cobalt,  and  ignited  in  the  oxidizing  flame,  a 
black,  or  grey  infusible  mass  is  produced. 

(c.)  Lime,  Oxide  of  Calcium  (CaO). — Lime  does  not  occur 
free  in  nature,  but  in  combination  with  acids,  chiefly  the  car 
bonic  and  sulphuric.  The  phosphate  occurs  principally  in 
bones.  The  hydrate  and  the  salts  of  lime  are  in  their  pro 
perties  similar  to  those  of  the  two  preceding  alkaline  earths. 
In  the  pure  state,  the  oxide  of  calcium  is  white;  it  slakes* 
produces  a  high  temperature,  and  falls  into  a  white  powder 
when  sprinkled  with  a  little  water.  It  is  now  a  hydrate, 
and  has  greatly  increased  in  volume.  The  hydrate  of  lime 
is  far  less  soluble  in  water  than  either  those  of  baryta  or 
strontia,  and  is  less  soluble  in  hot  water  than  in  cold.  Lime, 
its  hydrate  and  sulphide  of  calcium,  have  a  strong  alkaline 
reaction  upon  red  litmus  paper.  Lime  and  its  hydrate  are 
infusible,  but  produce  at  a  strong  red  heat  a  very  intense  and 
splendid  white  light,  while  the  hydrate  loses  its  water.  The 
carbonate  of  lime  is  also  infusible,  but  at  a  red  heat  the 
carbonic  acid  is  expelled,  and  the  residue  becomes  caustic, 


SPECIAL     REACTIONS.  119 

appears  winter,  and  produces  an  intenser  light.  The  sulphate 
of  lime  melts  with  difficulty,  and  presents  the  appearance  of  an 
enamelled  mass  when  cold.  By  Cheating  it  upon  charcoal  it 
fuses  in  the  reducing  flame,  and  is  reduced  to  a  sulphide.  This 
has  a  strong  hepatic  odor,  and  exerts  an  alkaline  reaction  upon 
red  litmus  paper.  By  exposing  lime,  or  its  compounds,  upon 
platinum  wire — or  as  a  small  splinter  of  the  mineral  in  the 
platinum  tongs — to  the  point  of  the  blue  flame,  a  purple  color, 
similar  to  that  of  lithia  and  strontia,  is  communicated  to  the 
external  flame,  but  this  color  is  not  so  intense  as  that  produced 
by  strontia,  and  appears  mixed  with  a  slight  tinge  of  yel 
low.  This  color  is  most  intense  with  the  chloride  of  calcium, 
while  the  carbonate  of  lime  produces  at  first  a  yellowish  color, 
which  becomes  red,  after  the  expulsion  of  the  carbonic  acid. 
Sulphate  of  lime  produces  the  same  color,  but  not  so  intense. 
Among  the  silicates  of  lime  only  the  tablespar  (3CaO, 
2Si03)  produces  a  red  color.  Fluorspar  (CaFl)  produces  a 
red  as  intense  as  pure  lime,  and  fuses  into  a  bead.  Phosphate 
and  borate  of  lime  produce  a  green  flame  which  is  only  charac 
teristic  of  their  acids.  The  presence  of  baryta  communicates 
a  green  color  to  the  flame.  The  presence  of  soda  produces 
only  a  yellow  color  in  the  external  flame. 

If  alcohol  is  poured  over  lime  or  its  compounds  and  inflamed, 
a  red  color  is  communicated  to  the  flame.  The  presence  of 
baryta  or  soda  prevents  this  reaction.  Lime  and  its  compounds 
do  not.  dissolve  much  by  fusion  with  carbonate  of  soda.  If  this 
fusion  is  effected  on  charcoal,  the  carbonate  of  soda  is  absorbed^ 
and  the  lime  remains  as  a  half-globular  infusible  mass  on  the  char 
coal.  This  is  what  distinguishes  lime  from  baryta  and  strontia, 
and  is  a  good  method  of  separating  the  former  from  the  latter. 
Lime  and  its  compounds  fuse  with  borax  in  the  oxidizing  and 
reducing  flames  to  a  clear  bead,  which  remains  clear  when 
cold,  but  when  overcharged  with  an  excess  or  heated  intermit, 
tiugly,  the  bead  appears,  when  cold,  crystalline  and  uneven,  and 
is  not  so  milk-white  as  the  bead  of  baryta  or  strontia,  produced 
under  the  same  circumstances. .  The  carbonate  of  lime  is  dis- 


120  THE    BLOWPIPE. 

solved  with  a  peculiar  hissing  noise.  Microcosrnic  salt  dissolves 
a  large  quantity  of  lime  into  a  clear  bead,  which  is  milky 
when  cold.  When  the  bead  has  been  overcharged  with  lime, 
by  a  less  excess,  or  by  an  intermittent  flame,  we  will  perceive  in 
the  bead,  when  cold,  fine  crystals  in  the  form  of  needles.  Lime 
and  its  compounds  form  by  ignition  with  nitrate  of  cobalt,  a 
black  or  greyish-black  infusible  mass. 

(d.)  Magnesia  (MgO). — Magnesia  occurs  in  nature  in  seve 
ral  minerals.  It  exists  in  considerable  quantity  combined  with 
carbonic,  sulphuric,  phosphoric,  and  silicic  acids,  etc.  Magnesia 
and  its  hydrate  are  white  and  very  voluminous,  scarcely  soluble 
in  hot  or  cold  water,  and  restores  moistened  red  litmus  paper 
to  its  original  blue  color.  Magnesia  and  its  hydrate  are 
infusible,  the  latter  losing  its  water  by  ignition.  The  carbonate 
of  magnesia  is  infusible,  loses  its  carbonic  acid  at  a  red  heat, 
and  shrinks  a  little.  It  now  exerts  upon  red  litmus  paper  an 
alkaline  reaction.  The  sulphate  of  magnesia,  at  a  red  heat, 
loses  its  water  and  sulphuric  acid,  is  entirely  infusible,  and 
gives  now  an  alkaline  reaction.  The  artificial  Astrachanit 
(NaO,  SO3  +  MgO,  S08  +  4HO)  fuses  easily.  When  fused  on 
charcoal,  the  greater  part  of  the  sulphate  of  soda  is  absorbed, 
and  there  remains  an  infusible  mass. 

Magnesia  and  its  compounds  do  not  produce  any  color  in  the 
external  flame,  when  heated  in  the  point  of  the  blue  flame. 
The  most  of  the  magnesia  minerals  yield  some  water  when 
heated  in  a  glass  tube  closed  at  one  end. 

Magnesia,  in  the  pure  state,  or  as  the  hydrate,  does  not  fuse 
with  soda.  Some  of  its  compounds  are  infusible  likewise  with 
soda,  and  swell  up  slightly,  while  others  of  them  melt  with 
soda  to  a  slightly  opaque  mass.  Some  few  (such  as  the  borate 
of  magnesia)  give  a  clear  bead  with  soda,  though  it  becomes 
slightly  turbid  by  cooling  when  saturated  with  magnesia,  and 
crystallizes  in  large  facets. 

Magnesia  and  its  compounds  give  beads  with  borax  and 
microcosmic  salt  similar  to  those  of  lime.  By  igniting  mag 
nesia  or  its  compounds  very  strongly  in  the  oxidizing  flame, 


SPECIAL    REACTIONS.  121 

moistening  with  nitrate  of  cobalt,  and  re-igniting  in  the 
oxidation  flame,  they  present,  after  a  continued  blowing,  a  pale 
flesh-color,  which  is  more  visible  when  cold.  It  is  indispensa 
ble  that  the  magnesia  compounds  should  be  completely  white  and 
free  of  colored  substances,  or  the  color  referred  to  cannot  be 
discerned.  In  general  the  reactions  of  magnesia  before  the 
blowpipe  are  not  sufficient,  and  it  will  be  necessary  to  confirm 
its  presence  or  absence  by  aid  of  reagents  applied  in  the  wet 
way. 


THIRD    GROUP. THE    EARTHS,  ALUMINA,  GLUCINA,    YTTRIA,    THORINA, 

AND    ZIRCONIA. 

The  substances  of  this  group  are  distinguished  from  the  pre 
ceding  by  their  insolubility  in  water,  in  their  pure  or  hydrated 
state — that  they  have  no  alkaline  reaction  upon  litmus  paper, 
nor  form  salts  with  carbonic  acid.  The  earths  are  not  volatile, 
and,  in  the  pure  state,  are  infusible.  They  cannot  be  reduced 
to  the  metallic  state  before  the  blowpipe.  The  organic  salts 
are  destroyed  by  ignition,  while  the  earths  are  left  in  the  pure 
state,  mixed  with  charcoal,  from  the  organic  acids.  The  most 
of  their  neutral  salts  are  insoluble  in  water;  the  soluble  neutral 
salts  change  blue  litmus  paper  to  red,  and  lose  their  acids  when 
ignited. 

(a.)  Alumina  (APO3). — This  earth  is  one  of  our  most  com 
mon  minerals.  It  occurs  free  in  nature  in  many  minerals,  as 
sapphire,  etc.;  or  in  combination  with  sulphuric  acid,  phos 
phoric  acid,  and  fluorine,  and  chiefly  silicates.  Pure  alum 
ina  is  a  white  crystalline  powder,  or  yellowish-white,  and 
amorphous  when  produced  by  drying  the  hydrate,  separated 
chemically  from  its  salts.  Alumina  is  quite  unalterable  in  the 
fire ;  the  hydrate,  however,  losing  its  water  at  a  low  red  heat. 
The  neutral  salts  of  alumina,  with  most  acids,  are  insoluble  in 
water.  Those  soluble  in  it  have  an  acid  reaction  upon  litmus 
paper,  changing  the  blue  into  red. 

6 


122  THE    BLOWPIPE. 

The  sulphates  of  alumina  eliminate  water  when  heated  in  a 
glass  tube  closed  at  one  end.  By  ignition,  sulphurous  acid 
(SO2)  is  given  off,  which  can  be  recognized  by  its  smell,  and 
by  its  acid  reaction  upon  blue  litmus  paper,  when  a  small  strip 
of  it  moistened  is  brought  within  the  orifice  of  the  tube;  an 
infusible  residue  is  left  in  the  tube. 

The  greater  part  of  the  alumina  compounds  give  off  water 
with  heat;  the  most  of  them  are  also  infusible,  except  a  few 
phosphates  and  silicates. 

Pure  alumina  does  not  fuse  with  carbonate  of  soda.  The 
sulphates,  when  exposed  upon  charcoal  with  soda  to  the  reduc 
ing  flame,  leave  a  hepatic  residue.  The  phosphates  melt  with 
a  little  soda,  with  a  hissing  noise,  to  a  semi-transparent  mass, 
but  they  are  infusible  with  the  addition  of  soda,  and  give  only 
a  tough  mass.  This  is  the  case,  likewise,  with  the  silicates  of 
alumina.  Fluoride  of  aluminium  melts  with  carbonate  of  soda  to 
a  clear  bead,  spreads  by  cooling,  and  appears  then  milk-white. 
Borax  dissolves  the  alumina  compounds  slowly  in  the  oxidizing 
and  reducing  flames  to  a  clear  bead,  which  is  also  clear  when 
cold,  or  heated  intermittingly  with  a  vacillating  flame.  The 
bead  is  turbid,  as  well  in  the  heat  as  the  cold,  when  an  excess 
of  alumina  is  present.  When  the  alumina  compound  is  added 
to  excess  in  the  powdered  form,  the  bead  appears  crystalline 
upon  cooling,  and  melts  again  with  great  difficulty. 

Alumina  and  its  compounds  are  slowly  dissolved  in  the 
microcosmic  salt  to  a  bead,  clear  in  both  flames,  and  when  hot 
or  cold.  When  alumina  is  added  to  excess,  the  undissolved 
portion  appears  semi-transparent.  Alumina  melts  with  bisul- 
phate  of  potash  into  a  mass  soluble  in  water.  When  the  pow 
dered  alumina  compounds  are  strongly  ignited  in  the  oxidizing 
flame,  then  moistened  with  nitrate  of  cobalt,  and  re-ignited 
in  the  oxidizing  flame,  an  infusible  mass  is  left,  which  appears, 
when  cooled,  of  an  intense  blue  color.  The  presence  of  colored 
metallic  oxides,  in  considerable  quantity,  will  alter  or  suppress 
this  reaction.  The  silicates  of  the  alkalies  produce,  in  a  very 
strong  heat)  or  continued  heat,  with  nitrate  of  cobalt,  a  pale 


SPECIAL     REACTIONS.  123 

blue  color.  The  blue  color  produced  by  alumina  is  only  dis 
tinctly  visible  by  daylight;  by  candle-light  it  appears  of  a  dirty 
violet  color. 

(b.)  Gludna.  (G203). — Glucina  only  occurs  in  a  few  rare 
minerals,  in  combination  with  silica  and  alumina.  It  is  white 
and  insoluble  in  the  pure  state,  and  its  properties  generally  are 
similar  to  those  of  alumina.  The  most  of  its  compounds  are 
infusible,  and  yield  water  by  distillation.  Carbonate  of  soda 
does  not  dissolve  glucina  by  ignition.  Silicate  of  glucica  melts 
with  carbonate  of  soda  to  a  colorless  globule.  Borax  and 
microcosmic  salt  dissolve  glucina  and  its  compounds  to  a  color 
less  bead  which,  when  overcharged  with  glucina,  or  heated  with 
the  intermittent  flame  appears,  after  cooling,  turbid  or  milk- 
white.  Glucina  yields,  by  ignition  with  nitrate  of  cobalt,  a 
black,  or  dark  grey  infusible  mass. 

(c,)  Ytlria  (YO)  occurs  only  in  a  few  rare  minerals,  and 
usually  in  company  with  terbium  and  erbium.  Its  reactions 
before  the  blowpipe  are  similar  to  the  preceding,  but  for  its 
detection  in  compounds  it  will  be  necessary  to  resort  to  analy 
sis  in  the  wet  way. 

(d.)  Zirconia  (Zr203). — This  substance  resembles  alumina 
in  appearance,  though  it  occurs  only  in  a  few  rare  minerals. 
It  is  in  the  pure  state  infusible,  and  at  a  red  heat  produces  such 
a  splendid  and  vivid  white  light  that  the  eyes  can  scarcely 
endure  it.  Its  other  reactions  before  the  blowpipe  are  analo 
gous  to  glucina.  Microcosmic  salt  does  not  dissolve  so  much 
zirconia  as  glucina,  and  is  more  prone  to  give  a  turbid  bead. 
Zirconia  yields  with  nitrate  of  cobalt,  when  ignited,  an  infusible 
black  mass.  To  recognize  zirconia  in  compounds  we  must  resort 
to  fluid  analysis. 

(e.)  Thor'ma  (ThO). — This  is  the  rarest  among  the  rare 
minerals.  In  the  pure  state  it  is  white  and  infusible,  and  will 
not  melt  with  the  carbonate  of  soda.  Borax  dissolves  thoriua 
slowly  to  a  colorless,  transparent  bead,  which  will  remain  so 
when  heated  with  the  intermittent  flame.  If  overcharged  with 
the  thorina,  the  bead  presents,  on  cooling,  a  milky  hue.  Micro- 


THE     BLOWPIPE. 


cosmic  salt  dissolves  the  thorina  very  tardily.  By  ignition 
with  nitrate  of  cobalt,  thorina  is  converted  into  an  infusible 
black  mass. 


CLASS  II. 

FOURTH  GROUP. CERIUM,  LANTHANIUM,  DIDYMIUM,  COLUMBIUM,  NIO 
BIUM,  PELOPIUM,  TITANIUM,  URANIUM,  VANADIUM,  CHROMIUM, 
MANGANESE. 

The  substances  of  this  group  cannot  be  reduced  to  the 
metallic  state,  neither  by  heating  them  per  se,  nor  by  fusing 
them  with  reagents.  They  give  by  fusion  with  borax  or  micro- 
cosmic  salt,  colored  beads,  while  the  preceding  groups  give 
colorless  beads. 

(a.)  Cerium  (Ce). — This  metal  occurs  in  the  oxidated  state 
in  a  few  rare  minerals,  and  is  associated  with  lanthanium  and 
didymium,  combined  with  fluorine,  phosphoric  acid,  carbonic 
acid,  silica,  etc.  When  reduced  artificially,  it  forms  a  grey 
metallic  powder. 

(a.)  Protoxide  of  Cerium  (CeO). — It  exists  in  the  pure  state 
as  the  hydrate,  and  is  of  a  white  color.  It  soon  oxidizes  and 
becomes  yellow,  when  placed  in  contact  with  the  air.  When 
heated  in  the  oxidation  flame,  it  is  converted  into  the  sesqui- 
oxide,  and  then  is  changed  into  light  brick-red  color.  In  the 
oxidation  flame  it  is  dissolved  by  borax  into  a  clear  bead,  which 
appears  of  an  orange  or  red  while  hot,  but  becomes  yellow 
upon  cooling.  When  highly  saturated  with  the  metal,  or  when 
heated  with  a  fluctuating  flame,  the  bead  appears  enamelled  as 
when  cold.  In  the  reduction  flame  it  is  dissolved  by  borax  to 
a  clear  yellow  bead,  which  is  colorless  when  cold.  If  too  much 
of  the  metal  exists  in  the  bead,  it  then  appears  enamelled  when 
cooled. 

Microcosmic  salt  dissolves  it,  in  the  oxidation  flame,  to  a, 
clear  bead,  which  is  colored  dark  yellow  or  orange,  but  loses 
its  color  when  cold.  In  the  reduction  flame  the  bead  is  color- 


SPECIAL    REASONS.  125 

less  when  either  hot  or  cold.  Even  if  highly  saturated  with 
the  metal,  the  bead  remains  colorless  when  cold.  By  fusing  it 
with  carbonate  of  soda  upon  charcoal  in  the  reduction  flame, 
the  soda  is  absorbed  by  the  charcoal,  while  the  protoxide  of 
the  metal  remains  as  a  light  grey  powder. 

(B.)  Sesquioxide  of  Cerium  (Ce203).— This  oxide,  in  the 
pure  state,  is  a  red  powder.  When  heated  with  hydrochloric 
acid,  it  produces  chlorine  gas,  and  is  dissolved  to  a  salt  of  the 
protoxide.  It  is  not  affected  by  either  the  flame  of  oxidation 
or  of  reduction;  when  fused  with  borax  or  microcosmic  salt,  it 
acts  like  the  protoxide.  It  does  not  fuse  with  soda  upon  char 
coal.  In  the  reduction  flame  it  is  reduced  to  the  protoxide, 
which  remains  of  a  light  grey  color,  while  the  soda  is  absorbed 
by  the  charcoal. 

(&.)  Lanthanium  (La.) — This  metal  is  invariably  associated 
with  cerium.  It  presents,  in  its  metallic  state,  a  dark  grey 
powder,  which  by  compression  acquires  the  metallic  lustre. 

The  oxide  of  lanthanium  (LaO)  is  white,  and  its  salts  are 
colorless.  Heated  upon  charcoal,  it  does  not  change  either  in 
the  oxidation  flame  or  that  of  reduction.  With  borax,  in  the 
flame  of  oxidation  or  reduction,  it  gives  a  clear  colorless  bead. 
This  bead,  if  saturated,  and  when  hot,  presents  a  yellow  appear 
ance,  but  is  clouded  or  enamelled  when  cold.  With  microcos 
mic  salt  the  same  appearance  is  indicated.  It  does  not  fuse 
with  carbonate  of  soda,  but  the  soda  is  absorbed  by  the  char 
coal,  while  the  oxide  remains  of  a  grey  color. 

(c.)  Didymium  (D). — This  metal  occurs  only  in  combination 
with  the  preceding  ones,  and  it  is  therefore,  like  them,  a  rare 
one. 

Oxide  of  Didymium  (DO). — This  oxide  is  of  a  brown  color, 
while  its  salts  present  a  reddish-violet  or  amethyst  color.  The 
oxide  is  infusible  in  the  oxidation  flame,  and  in  that  of  reduc 
tion  it  loses  its  brown  color  and  changes  to  grey.  With  borax 
in  the  oxidation  flame,  it  fuses  to  a  clear  dark  red  or  violet 
bead,  which  retains  its  clearness  when  highly  saturated  with 
the  oxide,  or  if  heated  with  a  fluctuating  flame. 


126  T  H  E      B  L  O  W  P  I  P  E  . 

The  reactions  with  rnicrocosmic  salt  are  the  same  as  with 
borax. 

It  does  not  melt  with  carbonate  of  soda  upon  charcoal,  but 
the  oxide  remains  with  a  grey  color,  while  the  soda  is  absorbed 
by  the  charcoal. 

(d.)  Columbium,  (Tantalum— -1 'a). — This  rare  metal  occurs 
quite  sparingly  in  the  minerals  tantalite,  yttrotantalite,  etc.,  as 
columbic  acid.  In  the  metallic  state,  it  presents  the  appear 
ance  of  a  black  powder,  which,  when  compressed,  exhibits  the 
metallic  lustre.  When  heated  in  the  air  it  is  oxidized  into 
columbic  acid,  and  is  only  soluble  in  hydrofluoric  acid,  yielding 
hydrogen.  It  is  oxidized  by  fusion  with  carbonate  of  soda  or 
potash. 

Columbic  Acid  (Ta303)  is  a  white  powder,  and  is  infusi 
ble.  When  heated  in  the  flame  of  oxidation  or  reduction,  it 
appears  of  a  light  yellow  while  hot,  but  becomes  colorless  when 
cold.  With  borax,  in  the  flames  of  oxidation  and  reduction,  it 
fuses  to  a  clear  bead,  which  appears  by  a  certain  degree  of 
saturation,  of  a  yellow  color  so  long  as  it  continues  hot,  but 
becomes  colorless  when  cold.  If  overcharged,  or  heated  with 
an  intermittent  flame,  it  presents  an  enamel  white  when  cool. 

It  melts  with  microcosmic  salt  quite  readily  in  both  of  the 
flames,  to  a  clear  bead,  which  appears,  if  a  considerable  quan 
tity  of  columbic  acid  be  present,  of  a  yellow  color  while  hot, 
but  colorless  when  cold,  and  does  not  become  clouded  if  the 
intermittent  flame  be  applied  to  it. 

With  carbonate  of  soda  it  fuses  with  effervescence  to  a  bead 
which  spreads  over  the  charcoal.  Melted  with  more  soda,  it 
becomes  absorbed  by  the  charcoal. 

It  yields,  moistened  with  a  solution  of  nitrate  of  cobalt,  and 
exposed  to  the  oxidation  flame  after  continued  blowing,  an  infu 
sible  mass,  presenting  while  hot  a  light  grey  color,  but  after 
being  cooled  that  of  a  light  red,  similar  to  the  color  presented 
by  magnesia  under  the  same  circumstances.  But  if  there  be 
some  alkali  mixed  with  it,  a  fusion  at  the  edges  will  be  mani 
fest,  and  it  will  yield  by  cooling  a  bluish-black  mass. 


SPECIAL    REACTIONS.  127 

(«.)  Niobium  (Ni). — This  metal  occurs  as  niobic  acid  in 
columbite  (tantalite).  Niobic  acid  is  in  its  properties  similar  to 
columbic  acid.  It  is  white  and  infusible.  By  heating  it  either 
in  the  flames  of  reduction  or  oxidation,  it  presents  as  long  as  it 
continues  hot,  a  greenish-yellow  color,  but  becomes  white  when 
cool.  Borax  dissolves  it  in  the  oxidation  flame  quite  readily  to 
a  clear  bead,  which,  with  a  considerable  quantity  of  niobic  acid, 
is  yellow  when  hot,  but  transparent  and  colorless  when  cold. 
A  saturated  bead  is  clear  when  either  hot  or  cold,  but  becomes 
opaque  when  heated  intermittingly. 

In  the  flame  of  reduction,  borax  is  capable  of  dissolving  more 
of  the  niobic  acid,  so  that  a  bead  overcharged  and  opaque  in 
the  oxidation  flame  appears  quite  clear  when  heated  in  the 
flame  of  reduction.  A  bead  overcharged  in  the  flame  of  reduc 
tion,  appears  by  cooling  dim  and  bluish-grey. 

Microcosmic  salt  dissolves  in  the  flame  of  oxidation  a  great 
quantity  of  it  to  a  clear  bead,  which  is  yellow  while  hot,  but 
colorless  when  cold. 

In  the  flame  of  reduction,  and  in  presence  of  a  considerable 
quantity  of  niobic  acid,  the  bead  appears  while  hot  of  a  light 
dirty  blue  color,  and  when  cold,  of  a  violet  hue  ;  but  by  the 
addition  of  more  niobic  acid,  the  bead,  when  hot,  is  of  a  dirty 
dark  blue  color,  and  when  cold,  of  a  transparent  blue.  In  the 
presence  of  the  oxides  of  iron,  the  bead  is,  while  hot,  of  a 
brownish-red  color,  but  changing  when  cool  to  a  dark  yellow. 

This  acid  fuses  with  an  equal  quantity  of  carbonate  of  soda 
upon  charcoal,  to  a  bead  which  spreads  very  quickly,  and  is 
then  infusible.  When  fused  with  still  more  soda,  it  is  absorbed. 

When  moistened  with  nitrate  of  cobalt,  and  heated  in  the 
flame  of  oxidation,  it  yields  an  infusible  mass  which  appears 
grey  when  hot,  and  dirty  green  when  cold  ;  but  if  the  heat  has 
been  too  strong,  it  is  fused  a  little  at  the  edges,  which  present 
a  dark  bluish-grey  color. 

Pelopium  (Pe). — This  metal  occurs  as  an  acid  in  the  mineral 
columbite  (tantalite),  and  is  very  similar  to  the  two  preceding 
metals. 


128  T  H  E      B  L  O  W  P  I  P  E  . 

(/.)  Pelopic  Acid  (PeOs). — This  acid  is  white,  and  appears 
yellow  when  heated,  but  resumes  its  white  color  when  cold. 
Borax  dissolves  it  in  the  oxidation  flame  to  a  clear  colorless 
bead,  which  appears,  when  overcharged  and  heated  intermit- 
tingly,  emanel-white  when  cold.  This  is  likewise  the  case  in 
the  flame  of  reduction,  but  when  overcharged  the  color  is  light 
grey,  when  the  bead  is  cooled. 

Microcosmic  salt  dissolves  it  in  the  flame  of  oxidation,  to  a 
clear  yellow  bead,  which  loses  its  color  when  cold.  In  the 
reduction  flame,  when  the  bead  is  highly  saturated,  a  violet- 
brown  color  is  produced.  In  presence  of  the  oxides  of  iron,  the 
reactions  are  like  those  of  niobic  acid.  With  carbonate  of 
soda,  the  reactions  are  similar  to  those  of  niobic  acid.  By 
heating  with  nitrate  of  cobalt,  it  yields  a  light  grey  infusible 
mass. 

(g.)  Titanium  (Ti). — This  metal  occurs  occasionally  in  the 
slags  of  iron  works,  in  the  metallic  state,  as  small  cubical  crys 
tals  of  a  red  color.  It  is  a  very  hard  metal,  and  very  infusible. 
Titanic  acid  occurs  in  nature  crystallized  in  anatase,  arkansite, 
brookite,  and  rutile.  Titanium  is  harder  than  agate,  entirely 
infusible,  and  loses  only  a  little  of  its  lustre,  which  can  be 
regained  by  fusion  with  borax.  It  does  not  melt  with  carbon 
ate  of  soda,  borax,  or  microcosmic  salt,  and  is  insoluble  in  every 
acid  except  the  hydrofluoric.  By  ignition  with  saltpetre  it  is 
converted  into  titanic  acid,  which  combines  with  the  potassium, 
forming  the  titanate  of  potassium. 

Titanic  Acid  (TiO2)  is  white,  insoluble,  and,  when  heated, 
it  appears  yellow  while  hot,  but  resumes  upon  cooling  its  white 
color. 

Borax  dissolves  it  in  the  oxidation  flame  to  a  clear  yellow 
bead,  which  when  cool  is  colorless.  When  overcharged,  or 
heated  with  the  intermitting  flame,  it  is  enamel-white  after 
being  cooled.  In  the  reduction  flame,  the  bead  appears 
yellow,  if  the  acid  exists  in  small  quantity,  but  if  more  be 
added,  then  it  is  of  an  orange,  or  dark  yellow,  or  even  brown. 
The  saturated  bead,  when  heated  intermittingly,  appears  when 


SPECIAL     REACTIONS.  129 

cold  of  an  enamelled  blue.  By  addition  of  the  acid,  and  by 
heating  the  bead  on  charcoal  in  the  reduction  flame,  it  becomes 
dark  yellow  while  hot,  but  dark  blue,  or  black  and  opaque 
when  cold.  This  bead  appears,  when  heated  intennittingly, 
of  a  light  blue,  and  when  cold,  enamelled. 

Microcosmic  salt  fuses  with  it  in  the  oxidation  flame  to  a 
clear  colorless  bead,  which  appears  yellow  only  in  the  presence 
of  a  quantity  of  titanic  acid,  though  by  cooling  it  loses  its 
color.  In  the  reduction  flame  this  bead  exhibits  a  yellow  color 
when  hot,  but  is  red  while  cooling,  and  when  cold  of  a  beauti 
ful  bluish-violet.  If  the  bead  is  overcharged,  the  color  becomes 
so  dark  that  the  bead  appears  opaque,  though  not  presenting 
an  enamel  appearance.  By  heating  the  bead  again  in  the  oxi 
dation  flame  the  color  disappears.  The  addition  of  some  tin 
promotes  the  reduction.  If  the  titanic  acid  contains  oxide 
of  iron,  or  if  some  is  added,  the  bead  appears,  when  cold, 
brownish-yellow,  or  brownish-red. 

By  fusion  with  carbonate  of  soda,  titanic  acid  is  dissolved 
with  effervescence  to  a  clear  dark  yellow  bead,  which  crystal 
lizes  by  cooling,  whereby  so  much  heat  is  eliminated,  that  the 
bead,  at  the  instant  of  its  crystallization,  glows  with  great 
brightness.  A  reduction  to  a  metal  cannot,  however,  be 
effected.  By  ignition  with  a  solution  of  nitrate  of  cobalt 
in  the  oxidation  flame,  it  yields  an  infusible  yellowish-green  mass. 

(h.)  Uranium  (U). — This  rare  metal  occurs  in  the  form  of 
protoxide  along  with  other  oxides,  in  the  mineral  pitch-Uende  ; 
as  peroxide  in  uranite  and  uran-mica,  associated  with  phos 
phoric  acid  and  lime. 

In  the  metallic  state  it  presents  the  appearance  of  a  dark 
grey  mass,  which  is  infusible,  and  remains  unchanged  when 
under  water,  or  when  exposed  to  dry  air,  but,  when  heated  in 
the  oxidation  flame,  it  becomes  oxidized,  with  lively  sparkling, 
to  a  dark  green  mass,  composed  of  the  protoxide  and  peroxide. 

The  protoxide  of  uranium  (UO)  is  black,  uncrystalline,  or 
forms  a  brown  powder.  When  exposed  to  heat  it  is  converted 
partially  into  peroxide,  when  it  has  a  dark  green  color. 


130  THE    BLOWPIPE. 

The  peroxide,  of  uranium  (U203)  is  of  an  orange  color, 
while  its  hydrate  is  of  a  fine  yellow  color,  and  in  the  form  of  a 
powder.  The  salts  are  yellow. 

By  heating  it  in  the  oxidation  flame,  it  acquires  a  dark  green 
color,  and  is  partly  reduced  to  protoxide.  In  the  reduction 
flame  it  presents  a  black  appearance,  and  is  there  completely 
reduced  to  protoxide. 

Borax  dissolves  it  in  the  oxidation  flame  to  a  clear  dark  yel 
low  bead,  which  is  colorless  when  cold,  if  the  metal  is  not  pre 
sent  in  great  quantity.  If  more  of  the  metal,  or  peroxide,  be 
added,  the  bead  changes  to  orange  when  hot,  and  light  yel 
low  when  cold.  When  heated  with  the  intermittent  flame, 
it  requires  a  large  quantity  of  the  peroxide  to  produce  an 
enamel  appearance  in  the  cooled  bead, 

In  the  flame  of  reduction  the  bead  becomes  of  a  dirty  greeii 
color,  being  partly  reduced  to  protoxide,  and  appears,  with  a 
certain  degree  of  saturation,  black,  when  heated  intermittingly, 
but  never  enamelled.  The  bead  appears  on  charcoal,  and  with 
the  addition  of  tin,  of  a  dark  green  color. 

It  fuses  with  microcosmic  salt  in  the  oxidation  flame  to  a 
clear  yellow  bead,  which  is  greenish-yellow  when  cold.  In  the 
reduction  flame  it  produces  a  beautiful  green  bead,  which 
increases  when  cold. 

When  fused  upon  charcoal  with  the  addition  of  tin,  its  color 
is  darker.  Carbonate  of  soda  does  not  dissolve  it,  although 
with  a  very  small  portion  of  soda  it  gives  indications  of  fusion, 
but  with  still  more  of  the  soda  it  forms  a  yellow,  or  light-brown 
mass,  which  is  absorbed  by  the  charcoal,  but  it  is  not  reduced 
to  the  metallic  state. 

(i.)  Vanadium  (V). — This  very  rare  mineral  is  found  in 
small  quantity  in  iron-ores,  in  Sweden,  and  as  vanadic  acid  in 
a  few  rare  minerals.  The  metal  presents  the  appearance  of  an 
iron-grey  powder,  and  sometimes  that  of  a  silver-white  mass. 
It  is  not  oxidized  either  by  air  or  water,  and  is  infusible. 

Vanadic  Acid  (VOS)  fuses  upon  platinum  foil  to  a  deep 
orange  liquid,  which  becomes  crystalline  after  cooling.  When 


SPECIAL    REACTIONS.  131 

fused  upon  charcoal,  one  part  of  it  is  absorbed,  while  the  rest 
remains  upon  the  charcoal  and  is  reduced  to  protoxide  similar 
in  appearance  to  graphite. 

A  small  portion  of  it  fuses  with  borax  in  the  oxidation  flame 
to  a  clear  colorless  bead,  which  appears,  with  the  addition  of 
more  vanadic  acid,  of  a  yellow  color,  but  changes  to  green 
when  cold. 

In  the  reduction  flame  the  bead  is  brown  while  hot,  but 
changes,  upon  cooling,  to  a  beautiful  sapphire-green.  At 
the  moment  of  crystallization,  and  at  a  degree  of  heat  by 
which  at  daylight  no  glowing  of  the  heated  mass  is  visible 
it  begins  to  glow  again.  The  glow  spreads  from  the  periphery 
to  the  centre  of  the  mass,  and  is  caused  by  the  heat  liberated 
by  the  sudden  crystallization  of  the  mass.  It  now  exhibits  an 
orange  color,  and  is  composed  of  needle  crystals  in  a  compact 
mass. 

Microcosmic  salt  and  vanadic  acid  fuse  in  the  oxidation 
flame  to  a  dark  yellow  bead  which,  upon  cooling,  loses  much 
of  its  color. 

In  the  reduction  flame  the  bead  is  brown  while  hot,  but, 
upon  cooling,  acquires  a  beautiful  green  color. 

Yanadic  acid  fuses  with  carbonate  of  soda  upon  charcoal, 
and  is  absorbed. 

(k.)  Chromium  (Cr)  occurs  in  the  metallic  state  only  in 
a  very  small  quantity  in  meteoric  iron,  but  is  frequently  found 
in  union  with  oxygen,  as  oxide  in  chrome  iron  ore,  and  as 
chromic  acid  in  some  lead  ores. 

In  the  metallic  state  it  is  of  a  light  grey  color,  with  but 
little  metallic  lustre,  very  hard,  and  not  very  fusible.  Acids 
do  not  act  upon  it,  except  the  hydrofluoric;  fused  with  nitre, 
it  forms  chromate  of  potassa.  It  is  unaltered  in  the  blowpipe 
flame. 

Sesquioxide  of  Chromium  (Cr303). — This  oxide  forms  black 
crystals  of  great  hardness,  and  is  sometimes  seen  as  a  green 
powder.  Its  hydrate  (Cra08  +  6HO)  is  of  a  bluish-grey 
color.  It  forms  with  acids  two  classes  of  isomeric  salts,  some 


132  THE     BLOWPIPE. 

of  which  arc  of  a  green  color,  and  the  others  violet-red  or  ame 
thyst.  The  neutral  and  soluble  salts  have  an  acid  reaction 
upon  blue  litmus  paper,  and  are  decomposed  by  ignition. 

Sesquioxide  of  chromium  in  the  oxidation  and  reduction 
flames  is  uuchangable.  When  exposed  to  heat,  the  hydrate 
loses  its  water,  and  gives  a  peculiarly  beautiful  flame.  In  the 
oxidation  flame  borax  dissolves  the  sesquioxide  of  chromium 
slowly  to  a  yellow  bead  (chromic  acid)  which  is  yellowish  green 
when  cold.  Upon  the  addition  of  more  of  the  oxide,  the  bead  is 
dark  red  while  hot,  but  changes  to  green  as  it  becorns  cold. 

In  the  reduction  flame  the  bead  is  of  a  beautiful  green  color, 
both  while  hot  and  when  cold.  It  is  here  distinguished  from 
vanadic  acid,  which  gives  a  brownish  or  yellow  bead  while  hot. 

With  microcosmic  salt  it  fuses  in  the  oxidation  flame  to  a 
clear  yellow  bead,  which  appears,  as  it  cools,  of  a  dirty-green 
color,  but  upon  being  cool  is  of  a  fine  green  color.  If  there  be 
a  superabundance  of  the  oxide,  so  that  the  microcosmic  salt 
cannot  dissolve  it,  the  bead  swells  up,  and  is  converted  into  a 
foamy  mass,  in  consequence  of  the  development  of  gases. 

In  the  reduction  flame  it  fuses  to  a  fine  green  bead.  The 
addition  of  a  little  tin  renders  the  green  still  deeper. 

Sesquioxide  of  chromium  fuses  with  carbonate  of  soda  upon 
platinum  foil  to  a  brown  or  yellow  bead,  which,  upon  cooling, 
appears  of  a  lighter  color  and  transparent  (chromate  of 
sodium). 

When  fused  with  soda  upon  charcoal,  the  soda  is  absorbed, 
and  the  green  oxide  is  left  upon  it,  but  is  never  reduced  to  the 
metallic  state. 

Chromic  Add  (CrO3)  crystallizes  in  the  form  of  deep  ruby 
red  needles.  It  is  decomposed  into  sesquioxide  and  oxygen 
when  heated.  This  decomposition  is  attended  with  a  very 
lively  emission  of  light,  but  this  is  not  the  case  if  the  chromic 
acid  has  been  attained  by  the  cooperation  of  an  aqueous  solu 
tion,  unless  the  reduction  is  effected  in  the  vapor  of  ammonia. 
Before  the  blowpipe  chromic  acid  produces  the  same  reactions 
as  the  sesquioxide. 


SPECIAL    REACTIONS.  133 

(/.)  Manganese  (Mn). — This  metal  occurs  in  considerable 
abundance,  principally  as  oxides,  less  frequently  as  salts,  and 
sometimes  in  combination  with  sulphur  and  arsenic.  It  is  found 
in  plants,  and  passes  with  them  into  the  animal  body.  In  the 
metallic  state,  it  is  found  frequently  in  cast  iron  and  steel.  It 
is  a  hard,  brittle  metal,  fusible  with  difficulty,  and  of  a  light 
grey  color.  It  tarnishes  upon  exposure  to  the  air  and  under 
water,  and  falls  into  a  powder. 

Protoxide  of  Manganese  exists  as  a  green  powder  ;  as  hydrate 
separated  by  caustic  alkalies,  it  is  white,  but  oxidizes  very 
speedily  upon  exposure  to  the  air.  The  protoxide  is  the  base 
of  the  salts  of  manganese.  These  salts,  which  are  soluble  in 
water,  are  decomposed  when  heated  in  the  presence  of  the  air — 
except  the  sulphate  (MnO,  SO3),  but  if  the  latter  is  ex 
posed  to  ignition  for  awhile,  it  then  ceases  to  be  soluble  in 
water,  or  at  least  only  sparingly  so. 

Sesquioxide  of  Manganese  (Mn203)  Occurs  very  spar 
ingly  in  nature  as  small  black  crystals  (Braunite)  which  give, 
when  ground,  a  brown  powder.  When  prepared  by  chemical 
process,  it  is  in  the  form  of  a  black  powder.  The  hydrate 
occurs  sometimes  in  nature  as  black  crystals  (manganite).  By 
digestion  with  acids,  it  is  dissolved  into  salts  of  the  protoxide. 
With  hydrochloric  acid,  it  yields  chlorine. 

The  prot-sesquioxide  of  manganese  (MnO  +  MnaOs)  occurs 
sometimes  in  black  crystals  (hausmannite) .  Prepared  artifi 
cially,  it  is  in  the  form  of  a  brown  powder. 

Peroxide  of  Manganese  (MnO2)  occurs  in  considerable 
abundance  as  a  soft  black  amorphous  mass,  or  crystallized  as 
pyrolusite,  also  reniforra  and  fibrous.  It  is  deprived  of  a  part 
of  its  oxygen  when  exposed  to  ignition.  It  eliminates  a  consi 
derable  quantity  of  chlorine  from  hydrochloric  acid,  and  is 
thereby  converted  into  chloride  of  manganese  (CIMn). 

Most  of  the  manganese  compounds  which  occur  in  nature 
yield  water  when  heated  in  a  glass  tube  closed  at  one 
end.  The  sesquioxide  and  peroxide  give  out  oxygen  when 
strongly  heated,  which  can  be  readily  detected  by  the 


134:  THE    BLOWPIPE. 

increased  glow  which  it  causes,  if  a  piece  of  lighted  wood  or 
paper  is  brought  to  the  mouth  of  the  tube.  The  residue  left  in 
the  tube  is  a  brown  mass  (MnO  +  Mn203). 

When  exposed  to  ignition  with  free  access  of  air,  all  man 
ganese  oxides  are  converted  into  (MnO-f  Mn203),  but  with 
out  fusion.  Such,  at  least,  is  the  statement  of  some  of  the 
German  chemists,  although  it  will  admit  perhaps  of  further 
investigation. 

Manganese  oxides  fuse  with  borax  in  the  oxidation  flame  to 
a  clear  and  intensely  colored  bead,  of  a  violet  hue  while  hot, 
but  changing  to  red  as  it  cools.  If  a  considerable  quantity  of 
the  oxide  is  added,  the  bead  acquires  a  color  so  dark  as  to 
become  opaque.  If  such  be  the  case,  we  have  to  press  it  flat, 
by  which  its  proper  color  will  become  manifest. 

In  the  reduction  flame  the  bead  is  colorless.  A  very  dark 
colored  bead  must  be  fused  upon  charcoal  with  the  addition  of 
some  tin.  The  bead  must  be  cooled  very  suddenly,  for  if  it 
cools  too  slowly,  it  then  has  time  to  oxidize  again.  This  may 
be  effected  by  pushing  it  off  the  platinum  wire,  or  the  charcoal, 
and  pressing  it  flat  with  the  forceps. 

The  oxides  of  manganese  fuse  with  microcosmic  salt  in  the 
oxidation  flame,  to  a  clear  brownish-violet  bead,  which  appears 
reddish-violet  while  cooling.  This  bead  does  not  become 
opaque  when  overcharged  with  manganese.  As  long  as  it 
is  kept  in  fusion  a  continued  boiling  or  effervescence  takes 
place,  produced  by  the  expulsion  of  oxygen,  in  consequence  of 
the  fact  that  the  microcosmic  salt  cannot  dissolve  much  sesqui- 
oxide,  while  the  rest  is  reduced  to  protoxide,  is  re-oxidated,  and 
instantly  again  reduced.  If  the  manganese  is  present  in  such  a 
minute  quantity  as  not  to  perceptibly  tinge  the  bead,  the  color 
may  be  made  to  appear  by  the  contact  of  a  crystal  of  nitre 
while  hot.  The  bead  foams  up  upon  the  addition  of  the  nitre, 
and  the  foam  appears,  after  cooling,  of  a  rose-red  or  violet 
color.  In  the  reduction  flame  the  bead  sometimes  becomes 
colorless. 

The  oxides  of  manganese  fuse  with  carbonate  of  soda  upon 


SPECIAL    REACTIONS.  135 

platinum  foil  or  wire,  to  a  clear  green  bead,  which  appears 
bluish-green  and  partially  opaque  when  cold  (manganate  of 
soda  NaO  +  MnO3).  A  very  minute  trace  of  manganese 
will  produce  this  green  color.  The  oxides  of  manganese  can 
not  be  reduced  upon  charcoal  with  carbonate  of  soda  before 
the  blowpipe.  The  soda  is  absorbed,  and  (MnO  +  Mn203) 
is  left. 

GROUP  FIFTH. IRON,  COBALT,  NICKEL. 

The  oxides  of  this  group  are  reduced  to  the  metallic  state 
when  fused  with  carbonate  of  soda  upon  charcoal  in  the  reduc 
tion  flame.  Metals  when  thus  reduced  form  powders,  are  not 
fusible  or  volatile  in  the  blowpipe  flame,  but  they  are  attracted 
by  the  magnet. 

Furthermore,  these  oxides  are  not  dissolved  by  carbon 
ate  of  soda  in  the  oxidation  flame,  but  they  produce  colored 
beads  with  borax  and  microcosmic  salt. 

(a.)  Iron. — It  occurs  in  great  abundance  in  nature.  It  is 
found  in  several  places  in  America  in  the  metallic  state,  and  it 
likewise  occurs  in  the  same  state  in  meteors.  It  occurs  chiefly 
as  the  oxide  (red  hematite,  brown  hematite,  magnetic  oxide, 
etc.),  and  frequently  in  combination  with  sulphur.  Iron  also 
forms  a  constituent  of  the  blood. 

Metallic  iron  is  of  a  grey  color,  and  presents  the  metallic 
lustre  vividly  when  polished.  It  is  very  ductile,  malleable,  and 
tenacious.  It  is  very  hard  at  common  temperatures,  but  soft 
and  yielding  at  a  red  heat. 

In  dry  and  cold  air,  iron  does  not  oxidize,  but  when  the  air 
is  dry  and  moist,  it  oxidizes  rapidly.  This  likewise  takes  place 
with  great  rapidity  when  the  metal  is  heated  to  redness. 
When  submitted  to  a  white  heat  iron  burns  with  brilliant 
scintillations. 

Protoxide  of  Iron  (FeO). — This  oxide  does  not  occur  pure 
in  nature,  but  in  union  with  the  peroxide  of  iron  and  other 
substances.  It  presents  the  form  of  a  black  powder,  and  has 


136  THE    B  LO  w  P  i  P  E. 

some  metallic  lustre,  is  brittle,  and  fuses  at  a  high  tempera 
ture  to  a  vitreous  looking  mass.  It  is  attracted  by  the  magnet, 
and  of  course  is  susceptible  of  becoming  magnetic  itself.  It 
forms  with  water  a  hydrate,  but  this  passes  so  rapidly  into  a 
state  of  higher  oxidation,  that  it  is  difficult  to  keep  it  in  the 
pure  state. 

Magnetic  Oxide  of  Iron  (FeO  +  Fe203). — This  peculiar 
oxide  is  of  a  dark  color,  and  is  magnetic,  so  that  tacks  or 
small  nails  adhere  to  it  when  brought  in  contact  with  it.  It  is 
the  variety  of  the  oxide  termed  "  loadstone."  It  is  found  fre 
quently  crystallized  in  octahedrons  in  Scandinavia  and  other 
places.  Magnetic  oxide  of  iron  is  produced  when  red-hot  iron 
is  hammered. 

Sesquioxide  of  Iron  (Fe203). — This  oxide  is  found  native  in 
great  abundance  as  red  hematite  and  specular  iron,  crystallized 
in  the  rhombic  form.  In  the  crystalline  state  it  is  of  a  blackish- 
grey  color,  and  possessed  of  the  metallic  lustre.  When  pow 
dered,  it  forms  a  brownish-red  mass.  When  artificially  prepared, 
it  presents  the  appearance  of  a  blood-red  powder.  It  is  not 
magnetic,  arid  has  less  affinity  for  acids  than  the  protoxide. 
Its  hydrate  is  found  native  as  brown  hematite. 

By  exposing  the  peroxide  of  iron  to  the  oxidation  flame,  it  is 
not  acted  upon,  but  in  the  reduction  flame  it  becomes  reduced 
to  the  magnetic  oxide. 

The  oxides  of  iron  are  dissolved  by  borax  in  the  oxidation 
flame  to  a  clear  dark-yellow  or  dark-red  bead,  which  appears 
lighter  while  cooling,  and  yellowish  when  cold.  In  the  presence 
of  a  very  small  quantity  of  iron,  the  bead  appears  colorless 
when  cold.  If  the  iron  is  increased,  the  bead  is  opaque  while 
cooling,  and  of  a  dirty  dark-yellow  color  when  cold.  In  the 
reduction  flame,  and  fused  upon  platinum  wire,  the  bead 
appears  dark  green  (FeO  +  Fe203).  By  the  addition  of 
some  tin,  and  fused  upon  charcoal,  the  bead  appears  bluish- 
green,  or  not  unlike  that  of  sulphate  of  iron. 

Microcosmic  salt  dissolves  the  oxides  of  iron  in  the  oxidation 
flame  to  a  clear  bead,  which,  bv  the  addition  of  a  considerable 


SPECIAL     REACTIONS.  137 

quantity  of  iron,  becomes  of  an  orange  color  while  hot,  but 
gets  lighter  while  cooling,  presenting  finally  a  greenish  hue, 
and  gradually  becoming  lighter,  till,  when  cold,  it  is  colorless. 
If  the  iron  is  increased,  the  hot  bead  presents  a  dark  red  color, 
but  while  cooling  a  brownish-red,  which  changes  to  a  dirty- 
green,  and,  when  cold,  to  a  brownish-red  color.  The  decrease 
of  the  color  during  the  transition  from  the  hot  to  the  cold  state 
is  still  greater  in  the  bead  formed  by  the  microcosmic  salt. 

In  the  reduction  flame  no  change  is  visible  if  the  quantity  of 
iron  be  small.  By  the  addition  of  more  iron,  the  hot  bead 
appears  red,  and  while  cooling,  changes  to  yellow,  then  green, 
and,  when  cold,  is  of  a  dull  red.  By  fusing  the  bead  on  char 
coal  with  a  small  addition  of  tin,  it  exhibits,  while  cooling,  a 
bluish-green  color,  but,  when  cold,  is  colorless. 

The  oxides  of  iron  are  not  dissolved  in  the  oxidation  flame 
by  fusion  with  carbonate  of  soda.  By  ignition  with  soda  upon 
charcoal  in  the  reduction  flame,  they  are  absorbed  and  reduced 
to  the  metallic  state.  Cut  out  this  portion  of  the  charcoal ; 
grind  it  with  the  addition  of  some  water  in  an  agate  mortar, 
for  the  purpose  of  washing  off  the  carbon  particles,  when  the 
iron  will  remain  as  a  grey  magnetic  powder. 

(b.)  Cobalt  (Co)  occurs  in  combination  with  arsenic  and 
sulphur,  and  associated  with  nickel  and  iron.  It  is  found  occa 
sionally  in  combination  with  selenium,  and  there  are  a  traces  of 
it  in  meteoric  iron.  In  the  metallic  state  it  is  of  a  light,  red 
dish-grey  color,  rather  brittle,  and  only  fusible  at  a  strong 
white  heat;  at  common  temperatures  it  is  unalterable  by  air  or 
water.  At  a  red  heat,  it  oxidizes  slowly  and  decomposes  water; 
at  a  white  heat  it  burns  with  a  red  flame.  Cobalt  is  soluble 
in  dilute  sulphuric  or  hydrochloric  acid  by  the  aid  of  heat, 
whereby  hydrogen  is  eliminated.  These  solutions  have  a  fine 
red  color.. 

Protoxide  of  Cobalt  (CoO). — It  is  an  olive-green  powder, 
but,  by  exposure  to  the  air,  it  becomes  gradually  brown.  Its 
hydrate  is  a  rich  red  powder.  The  solution  of  its  salts  is  red, 
but  the  aqueous  solution  is  often  blue. 


138  T  H  E      B  L  O  W  P  I  P  E  . 

When  heated  in  the  oxidation  flame,  the  protoxide  is  con 
verted  into  the  black  proto-sesquioxide  (CoO  +  Co203).  In  the 
reduction  flame  it  shrinks  and  is  reduced  without  fusion  to  the 
metallic  state.  It  is  now  attracted  by  the  magnet  and  acquires 
lustre  by  compression. 

Borax  dissolves  it  in  the  oxidation  flame,  and  produces  a 
clear,  intensely  colored  blue  bead,  which  remains  transparent 
and  of  the  same  beautiful  blue  when  cold.  This  blue  is  like 
wise  manifest  even  if  the  bead  be  heated  intermittingly.  If 
the  cobalt  exists  in  considerable  quantity,  the  color  of  the  bead 
is  so  intense  as  to  appear  almost  black. 

This  reaction  of  cobalt  is  so  characteristic  and  sensitive  that 
it  can  detect  a  minute  trace. 

With  microcosmic  salt  the  same  reaction  is  exhibited,  but 
not  so  sensitive,  nor  is  the  bead  so  intensely  colored  when  cold 
as  that  with  borax. 

By  fusion  with  carbonate  of  soda  upon  a  platinum  wire,  with 
a  very  small  portion  of  cobalt,  a  bright  red  colored  mass  is 
produced  which  appears  grey,  or  slightly  green  when  cold. 
By  fusion  upon  platinum  foil  the  fused  portion  floats  down  from 
the  sides,  and  the  foil  is  coated  around  the  undissolved  part, 
with  a  thin,  dark-red  sublimate.  When  fused  upon  charcoal, 
and  in  the  reduction  flame,  it  is  reduced  with  soda  to  a  grey 
powder,  which  is  attracted  by  the  magnet,  and  exhibits  the 
metallic  lustre  by  compression. 

Sesquioxide  of  Cobalt  (Co303). — It  is  a  dark  brown  powder. 
Its  hydrate  (2HO  +  Co203)  is  a  brown  powder.  It  is  soluble 
only  in  acetic  acid  as  the  acetate  of  the  sesquioxide.  All  other 
acids  dissolve  its  salts  to  protoxide,  the  hydrochloric  acid  pro 
ducing  chloric  gas.  By  ignition  in  the  oxidation  flame,  it  is 
converted  into  the  proto-sesquioxide  (CoO  +  Co203)  and  pro 
duces  with  reagents  before  the  blowpipe  the  same  reactions  as 
the  protoxide. 

(c.)  Nickel  (Ni). — This  metal  occurs  invariably  associated 
with  cobalt,  and  in  analogous  combinations,  chiefly  as  the  arse 
nical  nickel.  In  the  metallic  state  it  is  greyish,  silver-white, 


SPECIAL    REACTIONS.  139 

has  a  high  lustre,  is  hard,  and  malleable  both  cold  and  hot. 
At  common  temperatures,  it  is  unalterable  either  in  dry  or  moist 
air.  When  ignited,  it  tarnishes.  It  is  easily  dissolved  by  nitric 
acid,  but  very  slowly  by  dilute  sulphuric  or  hydrochloric  acid, 
producing  hydrogen. 

Protoxide  of  Nickel  (NiO). — It  is  in  the  form  of  small  grey 
ish-black  octahedrons,  or  a  dark,  greenish-grey  powder.  Its 
hydrate  is  a  green  powder.  Both  are  unalterable  in  the  air, 
and  are  soluble  in  nitric,  sulphuric,  and  hydrochloric  acids,  to 
a  green  liquid.  The  protoxide  is  the  base  of  the  salts  of  nickel, 
which  in  the  anhydrous  state  are  yellow,  and  when  hydrated  are 
green.  The  soluble  neutral  salts  change  blue  litmus  paper  to 
red.  By  ignition  in  the  oxidation  flame,  protoxide  of  nickel  is 
unaltered.  In  the  reduction  flame  and  upon  charcoal,  it 
becomes  reduced,  and  forms  a  grey  adherent  powder,  which  is 
infusible,  and  presents  the  metallic  lustre  by  compression,  and 
is  magnetic.  Borax  dissolves  it  in  the  oxidation  flame  very 
readily  to  a  clear  bead,  of  a  reddish-violet  or  dark  yellow  color, 
but  yellow  or  light  red  when  cold.  If  there  is  but  a  small 
quantity  of  the  oxide  present,  it  is  colorless.  If  more  of 
the  oxide  be  present,  the  bead  is  opaque  and  dark  brown,  and 
appears,  while  cooling,  transparent  and  dark  red.  By  the  addi 
tion  of  a  salt  of  potassa  (the  nitrate  or  carbonate)  a  blue  or  a 
dark  purple  colored  bead  is  produced.  The  borax  bead,  in  the 
reduction  flame,  is  grey,  turbid,  or  completely  opaque  from  the 
reduced  metallic  particles.  After  a  continued  blast,  the  bead 
becomes  colorless,  although  the  particles  are  not  fused.  If  the 
nickel  contains  cobalt,  it  will  now  be  visible  with  its  peculiar 
blue  color.  Upon  charcoal,  and  by  the  addition  of  some  tin, 
the  reduction  of  the  oxide  of  nickel  is  easily  effected,  while  the 
reduced  nickel  fuses  with  the  tin. 

The  oxide  of  nickel  is  dissolved  by  microcosmic  salt  in  the 
oxidation  flame  to  a  clear  bead,  which  appears  reddish  while 
hot,  but  yellow  and  sometimes  colorless  when  cooling.  If  a 
considerable  quantity  of  nickel  be  present  the  heated  bead  is 
of  a  brown  color,  but  orange  when  cooled.  In  the  reduction 


140  THE     BLOWPIPE. 

flame,  and  upon  platinum  wire,  the  color  of  the  bead  is  orange 
when  cold ;  but  upon  charcoal,  and  with  the  addition  of  a  little 
tin,  the  bead  appears  grey  and  opaque.  After  being  submitted 
to  the  blowpipe  flame  all  the  nickel  is  reduced,  and  the  bead 
becomes  colorless. 

Carbonate  of  soda  does  not  affect  it  in  the  oxidation  flame, 
but  in  the  reduction  flame  and  upon  charcoal,  it  is  absorbed 
and  reduced,  and  remains,  after  washing  off  the  carbon,  as  a 
white  metallic  powder,  which  is  infusible,  and  has  a  greater 
attraction  for  the  magnet  than  iron. 

Sesquiozide  of  Nickel  (Ni203). — It  is  in  the  form  of  a  black 
powder,  and  does  not  combine  with  other  substances,  unless  it 
is  reduced  to  the  protoxide.  It  exhibits  before  the  blowpipe 
the  same  behavior  as  the  protoxide. 

GROUP    SIXTH. — ZINC,    CADMIUM,    ANTIMONY,    TELLURIUM. 

The  substances  of  this  group  can  be  reduced  upon  charcoal 
by  fusion  with  carbonate  of  soda,  but  the  reduced  metals  are 
volatilized,  and  cover  the  charcoal  with  sublimates. 

(a.)  Zinc  (Zn). — This  metal  is  found  in  considerable  abun 
dance,  but  never  occurs  in  the  pure  metallic  state,  but  in  com 
bination  with  other  substances,  chiefly  as  sulphide  in  zinc 
blende,  as  carbonate  in  calamine,  and  as  the  silicate  in  the 
kieselzinc  ore;  also,  with  sulphuric  acid,  the  "vitriol  of  zinc." 

Zinc  is  of  a  bluish-white  color  and  metallic  lustre,  is  crys 
talline  and  brittle  when  heated  400°F.,  but  malleable  and  duc 
tile  between  200°  and  300°.  It  will  not  oxidize  in  dry  air,  but 
tarnishes  if  exposed  to  air  containing  moisture,  first  becomes 
grey,  and  then  passes  into  the  white  carbonate.  It  decom 
poses  in  water  at  a  glowing  heat.  It  is  dissolved  by  diluted 
acids,  while  hydrogen  is  eliminated.  It  melts  at  about  775°, 
and  distills  when  exposed  to  a  white  heat  in  a  close  vessel. 
When  heated  over  1000°  in  the  open  air,  it  takes  fire,  and 
burns  with  a  bluish-white  light,  and  with  a  thick  white  smoke 
of  oxide  of  zinc. 


SPECIAL     REACTIONS.  141 

Oxide  of  Zinc  (ZnO). — In  the  pure  state,  oxide  of  zinc  is  a 
white  powder,  infusible,  and  not  volatile.  It  is  readily  soluble 
in  acids  after  being  heated  strongly.  Its  soluble  neutral  salts, 
when  dissolved  in  water,  change  blue  litmus  paper  to  red.  Its 
salts,  with  organic  acids,  are  decomposed  by  ignition,  and  the 
carbonate  of  zinc  remains. 

The  oxide  of  zinc  turns  yellow  by  being  ignited  in  the  oxida 
tion  flame,  but  it  is  only  visible  by  daylight;  this  color  changes 
to  white  when  cold.  It  does  not  melt,  but  produces  a  strong 
light,  and  it  is  not  volatile. 

It  disappears  gradually  in  the  flame  of  reduction,  while  a 
white  smoke  sublimates  upon  the  charcoal.  This  sublimate  is 
yellow  while  hot,  but  changes  to  white  when  cold.  The  cause 
of  this  is,  that  the  oxide  is  reduced,  is  volatilized,  and  re-oxi 
dized,  by  going  through  the  external  flame  in  the  form  of  a 
metallic  vapor. 

Borax  dissolves  oxide  of  zinc  in  the  flame  of  oxidation  easily 
to  a  clear  bead,  which  is  yellow  while  hot,  and  colorless  when 
cold.  The  bead  becomes,  by  the  addition  of  more  oxide,  enam 
elled,  while  cooling.  If  the  bead  is  heated  with  the  intermit 
tent  flame,  it  is  milk-white  when  cold.  When  heated  in  the 
flame  of  reduction  upon  platinum  wire,  the  bead  at  first 
appears  opaque,  and  of  a  greyish  color,  but  becomes  clear 
again  after  a  continued  blast. 

When  heated  upon  charcoal  in  the  reduction  flame,  it  is 
reduced  to  a  metal;  but,  at  the  same  moment,  is  volatilized, 
and  sublimes  as  oxide  of  zinc  upon  the  charcoal,  about  one 
line's  distance  from  the  assay.  This  is  likewise  the  case  with 
the  microcosmic  salt,  except  that  it  is  more  easily  volatilized  in 
the  reduction  flame. 

Carbonate  of  soda  does  not  dissolve  the  oxide  of  zinc  in  the 
flame  of  oxidation.  In  the  reduction  flame  and  upon  charcoal, 
the  oxide  of  zinc  is  reduced  to  the  metallic  state,  and  is  volatil 
ized  with  a  white  vapor  of  the  zinc  oxide,  which  sublimes  on 
the  charcoal  and  exhibits  a  yellow  color  while  hot,  and  which 


142  THE     BLOWPIPE. 

changes  to  white  when  cold.  By  a  strong  heat  the  reduced 
zinc  burns  with  a  white  flame. 

Moistened  with  a  solution  of  cobalt  oxide,  and  heated 
strongly  in  the  flame  of  oxidation,  zinc  oxide  becomes  of  a 
yellowish-green  color  while  hot,  and  changes  to  a  beautiful 
green  color  when  cold. 

(ft.)  Cadmium  (Cd). — This  is  one  of  the  rare  metals.  It 
occurs  in  combination  with  sulphur  in  greenockite,  and  in  some 
ores  of  zinc.  It  was  detected  first  in  the  year  1818,  and  pre 
sents  itself  as  a  tin-white  metal  of  great  lustre,  and  susceptible 
of  a  fine  polish.  It  has  a  fibrous  structure,  crystallizes  easily 
in  regular  octahedrons,  presenting  often  the  peculiar  arbores 
cent  appearance  of  the  fern.  It  is  soft,  but  harder  and  more 
tenacious  than  tin;  it  can  be  bent,  filed,  and  easily  cut:  it 
imparts  to  paper  a  color  like  that  of  lead.  It  is  very  malleable 
and  ductile,  and  can  be  hammered  into  thin  leaves.  It  is  easily 
fused,  and  melts  before  it  glows  (450°).  At  a  temperature  not 
much  over  the  boiling  point  of  mercury,  it  begins  to  boil,  and 
distills,  the  vapor  of  the  metal  possessing  no  peculiar  odor.  It 
is  unalterable  in  the  air  for  a  long  time,  but  at  length  it  tar 
nishes  and  presents  a  greyish-white,  half  metallic  color.  This 
metal  easily  takes  fire  when  heated  in  the  air,  and  burns  with 
a  brownish-yellow  vapor,  while  it  deposits  a  yellow  sublimate 
upon  surrounding  bodies.  It  is  easily  soluble  in  acids  with  the 
escape  of  hydrogen,  the  solutions  being  colorless.  Its  salts, 
soluble  in  water,  are  decomposed  by  ignition  in  free  air.  Its 
soluble  neutral  salts  change  blue  litmus  paper  to  red.  The 
salts,  insoluble  in  water,  are  readily  dissolved  in  acids. 

Oxide  of  Cadmium  (CdO). — This  oxide  is  of  a  dark  orange 
color.  It  does  not  melt,  and  is  not  volatile,  not  even  at  a  very 
high  temperature.  Its  hydrate  is  white,  loses  in  the  heat  its 
hydratic  water,  and  absorbs  carbonic  acid  from  the  air  when  it 
is  kept  in  open  vessels. 

Cadmium  oxide  is  unaltered  when  exposed  upon  platinum 
wire  in  the  flame  of  oxidation.  When  heated  upon  charcoal  in 
the  flame  of  reduction  it  disappears  in  a  very  short  time,  while 


SPECIAL     REACTIONS.  143 

the  charcoal  is  coated  with  a  dark  orange  or  yellow  powder, 
the  color  of  which  is  more  visible  after  it  is  cooled.  The  por 
tions  of  this  sublimate  furthest  from  the  assay  present  a 
visible  iridescent  appearance.  This  reaction  of  cadmium  is  so 
characteristic  and  sensitive  that  minerals  (for  instance,  cala- 
rnine,  carbonate  of  zinc)  which  contains  from  one  to  five 
per  cent,  of  carbonate  of  cadmium,  will  give  a  dark  yellowish 
ring  of  cadmium  oxide,  a  little  distance  from  the  assay,  after 
being  exposed  for  a  few  moments  to  the  flame  of  reduction. 
This  sublimate  is  more  visible  when  cold,  and  is  produced  some 
time  previous  to  the  reduction  of  the  zinc  oxide.  If  a  vapor  of 
the  latter  should  appear,  it  indicates  that  it  has  been  exposed 
too  great  a  length  of  time  to  the  flame. 

Borax  dissolves  a  considerable  quantity  of  cadmium  oxide 
upon  a  platinum  wire  to  a  clear  yellow  bead,  which,  when  cold, 
is  almost  colorless.  If  the  bead  is  nearly  saturated  with  the 
cadmium  oxide,  it  appears  milk-white  when  intermittingly 
heated.  If  the  bead  is  completely  saturated,  it  retains  its 
opalescent  appearance.  Upon  charcoal,  and  in  the  flame  of 
reduction,  the  bead  intumesces,  the  cadmium  oxide  becomes 
reduced  to  metal  ;  this  becomes  volatilized  and  re-oxidized,  and 
sublimes  upon  the  charcoal  as  the  yellow  cadmium  oxide. 

In  the  oxidation  flame,  microcosmic  salt  dissolves  a  large 
quantity  of  it  to  a  clear  bead,  which,  when  highly  saturated  and 
while  hot,  is  yellowish  colored,  but  colorless  when  cold.  By 
complete  saturation,  the  bead  is  enamel-white  when  cold. 

Upon  charcoal,  in  the  flame  of  reduction,  the  bead  is  slowly 
and  only  partially  reduced,  a  scanty  sublimate  being  produced 
on  the  charcoal.  The  addition  of  tin  promotes  the  reduction. 

Carbonate  of  soda  does  not  dissolve  cadmium  oxide  in  the 
oxidation  flame.  In  the  reduction  flame,  upon  charcoal,  it  is 
reduced  to  metal,  and  is  volatilized  to  a  red-brown  or  dark, 
red  sublimate  of  cadmium  oxide  upon  the  charcoal,  at  a  little 
distance  from  the  assay  the  charcoal  presenting  the  character 
istic  iridescent  appearance.  This  reaction  is  still  more  sensitive 
if  the  cadmium  oxide  is  heated  per  se  in  the  reduction  flame. 


144  THE     BLOWPIPE. 

Antimony  (Sb). — This  metal  is  found  in  almost  every  coun 
try.  It  principally  occurs  as  the  tersulphide  (SbS8),  either 
pure  or  combined  with  other  sulphides,  particularly  with  basic 
sulphides.  Sometimes  it  occurs  as  the  pure  metal,  and  rarer  in 
a  state  of  oxidation  as  an  antimonious  acid  and  as  the  oxysul- 
phide. 

In  the  pure  state,  antimony  has  a  silver-white  color,  with 
much  lustre,  and  presents  a  crystalline  structure.  The  commer 
cial  and  impure  metal  is  of  a  tin-white  color,  and  may  fre 
quently  be  split  in  parallel  strata.  It  is  brittle  and  easily 
pulverized.-..  It  melts  at  a  low  red  heat  (810°),  is  volati 
lized  at  a  white  heat,  and  can  be  distilled.  At  common  tem 
peratures  it  is  not  affected  by  the  air.  At  a  glowing  heat  it 
takes  fire,  and  burns  with  a  white  flame,  and  with  white  fumes, 
forming  volatile  antimonious  acid.  Common  acids  oxidize 
antimony,  but  dissolve  it  slightly.  It  is  soluble  in  aqua  regia 
(nitro-hydrochloric  acid). 

Sesquioxide  of  Antimony  (Sb208). — In  the  pure  state  this 
oxide  is  a  white  powder,  is  fusible  at  a  dull  red  heat  to  a 
yellow  liquid,  which,  after  cooling,  is  greyish-white  and  crys 
talline.  If  it  is  heated  excluded  from  the  air,  it  can  be 
volatilized  completely;  it  sublimes  in  bright  crystals  having  the 
form  of  needles.  It  occurs  sometimes  in  nature  as  white  and 
very  bright  crystals.  It  takes  fire  when  heated  in  the  open 
air,  and  burns  with  a  white  vapor  to  antimonious  acid.  It 
fuses  with  the  ter-sulphide  of  antimony  to  a  red  bead.  It  is 
distinguished  from  the  other  oxides  of  antimony  by  the  readi 
ness  with  which  it  is  reduced  to  the  metallic  state  upon  char 
coal,  and  by  its  easy  fusibility  and  volatility. 

The  sesquioxide  is  the  base  of  some  salts — for  instance, 
the  tartar  emetic.  It  is  not  soluble  in  nitric  acid,  but  is 
soluble  in  hydrochloric  acid.  This  solution  becomes  milky  by 
the  addition  of  water.  A  part  of  the  salts  of  the  sesquioxide 
of  antimony  are  decomposed  by  ignition.  The  haloid  salts  are 
easily  volatilized,  without  decomposition.  Its  soluble  neutral 
salts  change  blue  litmus  paper  to  red,  and  are  converted,  by 


SPECIAL     REACTIONS. 

admixture  of  water,  into  insoluble  basic  and  soluble  acid 
salts. 

Antimonious  acid  (antimoniate  of  sesquioxide  of  antimony, 
Sb203  +  Sb20B)  is  of  a  white  color,  but,  when  heated,  of  a  light 
yellow  color,  but  changes  to  white  again  when  cold.  It  is 
infusible  and  unaltered  by  heat.  It  forms  a  white  hydrate, 
and  both  are  insoluble  in  water  and  nitric  acid.  It  is  partly 
soluble  in  hydrochloric  acid,  with  the  application  of  heat.  The 
addition  of  water  causes  a  precipitate  in  this  solution. 

Antimonic  Acid  (Sb206). — In  the  pure  state  this  acid  is  a 
light  yellow-colored  powder.  Its  hydrate  is  white,  and  is 
iusoluble  in  water  and  nitric  acid.  It  is  sparingly  soluble 
in  hot  concentrated  hydrochloric  acid.  It  forms  salts  with 
every  base,  some  of  which  are  insoluble,  and  others  sparingly 
so.  Notwithstanding  that  antimonic  acid  is  insoluble  in  water, 
it  expels  the  carbonic  acid  from  the  solutions  of  the  carbonates 
of  the  alkalies.  Antimonic  acid  and  its  hydrate  changes  moist- 
tened  blue  litmus  paper  to  red. 


Behavior  of  Antimony  and  its  Oxides  before  the,  Blowpipe. 

Metallic  Antimony  fuses  easily  upon  charcoal.  When  heated 
to  glowing,  and  then  removed  from  the  flame,  it  continues  to 
glow  for  awhile,  and  produces  a  thick  white  smoke.  The 
vapor  crystallizes  gradually,  and  coats  the  assay  with  small 
crystals  which  iridesce  like  mother  of  pearl  (sesquioxide  of 
antimony).  It  is  not  volatile  at  the  temperature  of  melted 
glass.  Ignited  in  an  open  glass  tube,  it  burns  slowly  with  a 
white  vapor,  which  condenses  upon  the  cool  part  of  the  tube,  and 
exhibits  some  indications  of  crystallization.  This  vapor  consists 
of  the  sesquioxide,  and  can  be  driven  by  heat  from  one  place 
to  another,  without  leaving  a  residue.  If  the  metallic  antimony 
contains  sulphide  of  antimony,  there  is  a  corresponding  por 
tion  of  antimonious  acid  produced,  which  remains  as  a  white 
sublimate  after  the  sesquioxide  is  removed. 

T 


THE     BLOWPIPE. 

Sesquitxide,  of  antimony  melts  easily,  and  sublimes  as  a  white 
vapor.  It  may  be  prepared  by  precipitating  and  drying. 
When  heated,  it  takes  fire  previous  to  melting,  glows  like 
tinder,  and  is  converted  into  antimonious  acid,  which  is  now 
infusible.  When  heated  upon  charcoal  in  the  flame  of  reduc 
tion,  it  is  reduced  to  the  metallic  state,  and  partly  volatilized. 
A  white  vapor  sublimates  upon  the  charcoal,  while  the  external 
flame  exhibits  a  greenish-blue  color.  Antimonious  acid  is  infu 
sible,  produces  a  strong  light,  and  is  diminished  in  volume 
when  heated  in  the  external  flame,  during  which  time  a  dense 
white  vapor  sublimes  upon  the  charcoal.  It  is  not,  however, 
in  this  manner  reduced  to  the  metallic  state  like  the  sesqui- 
oxide. 

Antimonic  add,  when  first  heated,  becomes  white,  and  is 
converted  into  antimonious  acid.  Hydrated  antimonic  acid, 
which  is  originally  white,  appears  at  first  yellow  while  giving 
off  water,  and  then  becomes  white  again,  while  oxygen  is 
expelled,  and  it  is  converted  into  antimonious  acid. 

The  oxides  of  antimony  produce,  with  blowpipe  reagents,  the 
following  reactions  :  borax  dissolves  oxides  of  antimony  in  the 
oxidation  flame  in  considerable  quantity  to  a  clear  bead,  which 
is  yellow  while  hot,  but  colorless  when  cold.  If  the  bead  is 
saturated,  a  part  of  the  oxide  is  volatilized  as  a  white  vapor. 
Upon  charcoal,  in  the  oxidation  flame,  it  is  completely  vola 
tilized,  and  the  charcoal  is  covered  with  a  white  sublimate. 
Heated  upon  charcoal  in  the  reducing  flame,  the  bead  is  of  a 
greyish  color,  and  partially,  if  not  wholly  opaque,  from  the  pre 
sence  of  reduced  metallic  particles.  A  continued  heat  will 
volatilize  them,  and  the  bead  becomes  clear.  The  addition  of 
tin  promotes  the  reduction. 

Microcosmic  salt  dissolves  the  compounds  of  antimony  in  the 
flame  of  oxidation  with  intumescence,  to  a  clear  light-yellow 
colored  bead,  which  when  cold  is  colorless.  Heated  upon 
charcoal  in  the  reduction  flame,  the  bead  is  first  turbid,  but 
soon  becomes  transparent.  The  addition  of  tin  renders  the 
bead  greyish  while  cooling,  but  a  continued  blast  renders  it 


SPECIAL     REACTIONS.  14/T 

transparent.  Soda  dissolves  the  compounds  of  antimony  upon 
platinum  wire  in  the  oxidation  flame,  to  a  clear  colorless  bead, 
which  is  white  when  cold. 

Upon  charcoal,  both  in  the  oxidation  and  reduction  flames, 
the  antimony  compounds  are  readily  reduced  to  the  metal, 
which  is  immediately  volatilized,  and  produces  a  white  incrust 
ation  of  oxide  of  antimony  upon  the  charcoal.  If  the  anti 
mony  compounds  are  heated  upon  charcoal  in  the  flame  of 
reduction,  with  a  mixture  of  carbonate  of  soda  and  cyanide 
of  potassium  (KCy),  there  are  produced  small  globules  of 
metallic  antimony.  At  the  same  time,  a  part  of  the  reduced 
metal  is  volatilized  (this  continues  after  the  assay  is  removed 
from  the  flame)  and  re-oxidized.  A  white  incrustation  ap 
pears  upon  the  charcoal,  and  the  metallic  globules  are 
covered  with  small  white  crystals.  If  this  white  sublimate 
upon  the  charcoal  is  moistened  with  a  solution  of  cobalt- 
oxide,  and  exposed  to  the  reduction  flame,  a  part  of  it  is 
volatilized,  while  the  other  part  passes  into  higher  oxidation, 
and  remains,  after  cooling,  of  a  dirty  dark-green  color. 

(d.)  Tellurium  (Te). — This  is  one  of  the  rare  metals.  It 
occurs  very  seldom  in  the  metallic  state,  but  often  with  bis 
muth,  lead,  silver,  and  gold.  Tellurium,  in  the  pure  state,  is 
silver-white,  very  bright,  of  a  foliated  or  lamellar  structure, 
brittle,  and  easily  triturated.  It  is  inclined  to  crystallize.  It  is 
soluble  in  concentrated  sulphuric  acid  without  oxidation.  The 
solution  is  of  a  fine  purple  color,  and  gives  a  precipitate  with 
the  addition  of  water. 

Tellurium  in  the  Metallic  form. — By  the  aid  of  heat  it  is 
oxidized  in  sulphuric  acid,  a  portion  of  the  oxygen  of  the  acid 
oxidizing  the  metal,  while  sulphurous  acid  gas  escapes.  This 
solution  is  colorless,  and  is  tellurous  acid,  dissolved  in  sul 
phuric  acid.  It  melts  at  a  low  red  heat,  and  volatilizes  at  a 
higher  temperature.  If  tellurium  is  heated  with  free  access  of 
air,  it  takes  fire,  and  burns  with  a  blue  color,  the  flame  being 
greenish  at  the  edges,  while  a  thick  white  vapor  escapes,  which 
hus  a  feeble  acidulous  odor. 


148  THE     BLOWPIPE. 

Tdlurous  Add  (TeOa)  is  of  a  fine,  granulous,  crystalline  or 
white  earthy  mass,  which  is  partly  soluble  in  water.  The 
solution  has  a  strong  metallic  taste,  and  an  acid  reaction  upon 
litmus  paper.  Heated  in  a  tube  closed  at  one  end  until  it 
begins  to  glow,  it  fuses  to  a  yellow  liquid  which  is  colorless, 
crystalline,  and  opaque  when  cold.  Beads  of  it  remain  usually 
transparent  like  glass.  Heated  upon  platinum  wire  in  the 
flame  of  oxidation,  it  melts,  and  is  volatilized  as  a  white  vapor. 
When  heated  upon  charcoal  in  the  oxidation  flame,  it  melts, 
and  is  reduced  to  the  metallic  state,  but  volatilizes  and  a  sub 
limate  of  white  tellurous  acid  is  formed  upon  the  charcoal. 
The  edge  of  this  deposit  is  usually  red  or  dark-yellow. 

Heated  upon  charcoal  in  the  flame  of  reduction,  it  is  rapidly 
reduced,  the  external  flame  exhibiting  a  bluish-green  color. 

Borax  dissolves  it  in  the  oxidation  flame  upon  platinum  wire 
to  a  clear  colorless  bead  which  turos  grey  when  heated  upon 
charcoal,  through  the  presence  of  reduced  metallic  particles. 
Upon  charcoal,  in  the  reduction  flame,  the  bead  is  grey,  caused 
by  the  reduced  metal.  After  a  continued  blast,  tellurium  is 
completely  volatilized,  and  the  bead  appears  clear  again,  while 
a  white  sublimate  is  deposited  upon  the  charcoal. 

With  microcosmic  salt,  the  same  reactions  are  produced. 

With  carbonate  of  soda,  tellurous  acid  fuses  upon  platinum 
wire  to  a  clear  colorless  bead,  which  is  white  when  cold. 
Upon  charcoal  it  is  reduced,  and  forms  tellur-sodium,  which  is 
absorbed  by  the  charcoal,  and  metallic  tellurium,  which  is 
volatilized,  and  deposits  upon  the  charcoal  a  white  incrusta 
tion  (tellurous  acid). 

If  tellurous  acid,  finely  powdered  charcoal,  and  carbonate 
of  soda  are  mixed  together,  and  the  mixture  be  well  ignited  in 
a  closed  tube,  until  fusion  is  effected,  and  a  few  drops  of  boiled 
water  are  brought  into  the  tube,  they  are  colored  purple,  indi 
cating  the  presence  of  tdlur-sodium. 

Telluric  Add  (TeOs)  forms  six-sided  prismatic  crystals.  It 
has  not  an  acid,  but  rather  a  metallic  taste.  It  changes  blue 
litmus  paper  to  red  ;  is  slowly  soluble  in  water,  and  rather 


S  P  K  C  I  A  L       lv  E  A  C    T  I  O  N  S  .  14:9 

sparingly.  Exposed  to  a  high  temperature,  but  not  until 
glowing,  the  crystalline  acid  loses  its  water,  and  acquires  an 
orange  color,  but  still  it  preserves  its  crystalline  form,  although 
no  longer  soluble  in  water,  and  is  in  fact  so  much  changed  in 
its  properties  as  to  present  the  instance  of  an  isomeric  modifi 
cation. 

If  telluric  acid  is  heated  gently  in  a  closed  tube,  it  loses 
water  and  turns  yellow.  Heated  still  more  strongly,  it  becomes 
milk-white,  oxygen  is  expelled,  and  it  is  converted  into  tellu- 
rous  acid.  The  presence  of  oxygen  can  be  recognized  by  the 
more  lively  combustion  which  an  ignited  splinter  of  wood 
undergoes  when  held  in  it.  Telluric  acid  produces  the  same 
reactions  with  the  blowpipe  reagents  as  tellurous  acid. 


SEVENTH    GROUP. LEAD,  BISMUTH,  TIN. 

The  oxides  of  these  metals  are  also  reduced  to  the  metallic 
state  by  fusion  with  soda  upon  charcoal  in  the  flame  of  reduc 
tion,  but  they  are  volatilized  only  after  a  continued  blast,  and 
a  sublimate  is  thrown  upon  the  charcoal. 

(a.)  Lead  (Pb). — This  metal  occurs  in  considerable  quanti 
ty  in  nature,  chiefly  as  galena  or  lead-glance  (sulphide  of 
lead).  Likewise,  but  more  rarely,  as  a  carbonate  ;  also  as  a 
sulphate,  and  sometimes  combined  with  other  acids  and  metals. 

In  the  metallic  state,  lead  is  of  a  bluish-grey  color,  high  lus 
tre,  and  sp.  gr.  11 '4.  It  is  soft,  and  communicates  a  stain  to 
paper.  It  is  malleable,  ductile,  but  has  very  little  tenacity.  It 
melts  at  about  612°.  Exposed  to  the  air  it  soon  tarnishes,  being 
covered  with  a  grey,  matter,  which  some  regard  as  a  suboxide 
(Pb20),  and  others  as  simply  a  mixture  of  lead  and  protoxide. 
At  a  glowing  heat  it  is  oxidized  to  a  protoxide,  and  at  a  white 
heat  it  is  volatilized.  It  is  insoluble  in  most  acids.  It  is,  how 
ever,  soluble  in  nitric  acid,  but  without  decomposing  water. 

(L.)  Protoxide  of  Lead  (PbO). — It  is  an  orange-colored 
powder,  which  melts  at  a  glowing  temperature,  and  forms  a 


150  THE    BLOWPIPE. 

lamellar  mass  after  cooling.  Protoxide  of  lead  absorbs  oxygen 
from  the  atmosphere  while  melting,  which  is  given  off  again  by 
cooling.  Being  exposed  for  a  longer  while  to  the  air,  it  absorbs 
carbonic  acid  and  water,  and  becomes  white  on  the  surface. 
It  is  soluble  in  nitric  acid  and  caustic  alkalies.  It  forms  with 
most  acids  insoluble  salts.  It  is  slightly  soluble  in  pure  water, 
but  not  in  water  which  contains  alkaline  salts.  This  hydrate 
is  white. 

(j3.)  Red  Oxide  of  Lead  (Pb02,PbO).— It  forms  a  puce-colored 
powder.  It  is  insoluble  in  caustic  alkalies.  Hydrochloric  acid 
dissolves  it  and  forms  a  yellow  liquid,  which  is  soon  decomposed 
into  chloride  of  lead  and  chlorine.  It  is  reduced  by  ignition  to 
the  protoxide. 

(y.)  Peroxide  of  Lead  (PbO2). — It  is  a  dark-brown  powder. 
It  yields  with  hydrochloric  acid  the  chloride  of  lead  and  chlorine 
gas.  When  heated  it  liberates  oxygen,  and  is  reduced  to  the 
protoxide. 

Lead  combinations  give  the  following  reactions  before  the 
blowpipe  :  Metallic  lead  tarnishes  when  heated  in  the  oxidation 
flame,  and  is  instantly  covered  with  a  grey  matter,  consisting  of 
the  protoxide  and  the  metal.  It  fuses  quickly,  and  is  then  co 
vered  with  a  yellowish-brown  protoxide  until  all  the  lead  is 
converted  into  the  protoxide,  which  melts  to  a  yellow  liquid. 
In  the  reduction  flame  and  upon  charcoal,  it  is  volatilized,  while 
the  charcoal  becomes  covered  with  a  yellow  sublimate  of  oxide. 
A  little  distance  from  the  assay,  this  sublimate  appears  white 
(carbonate  of  lead).  Protoxide  of  lead  melts  in  the  flame  of 
oxidation  to  a  beautiful  dark  yellow  bead.  In  the  flame  of  re 
duction,  and  upon  charcoal,  it  is  reduced  with  intumescence  to 
metallic  lead,  which  is  volatilized  by  a  continued  blast,  and  sub 
limates  on  charcoal,  as  mentioned  above. 

Red  oxide  of  lead  turns  black  when  heated  in  the  glass  tube 
closed  at  one  end,  and  liberates  oxygen,  which  is  easily  detected 
by  the  introduction  of  an  ignited  splinter,  when  a  more  lively 
combustion  of  the  wood  proves  the  presence  of  uncombiued 
oxygen.  The  red  oxide  in  this  case  is  reduced  to  the  protoxide. 


SPECIAL    REACTIONS.  151 

Heated  upon  platinum  foil,  it  first  turns  black,  is  reduced  to  the 
protoxide,  and  melts  into  a  dark  yellow  liquid.  In  the  reduc 
tion  flame,  upon  charcoal,  it  is  reduced  to  the  metal  with  intu 
mescence.  After  a  continued  blast,  a  yellow  sublimate  of  pro 
toxide  is  produced  upon  the  charcoal,  and  at  a  little  distance  off, 
around  this  sublimate,  a  white  one  of  carbonate  of  lead  is  pro 
duced.  This  sublimate  disappears  when  touched  by  the  flame 
of  reduction,  while  it  communicates  an  azure  blue-tinge  to  the 
external  flame.  This  is  likewise  the  case  with  the  peroxide  of 
lead. 

The  different  oxides  of  lead  produce  with  the  blowpipe  re 
agents  the  same  reactions. 

Borax  dissolves  lead  compounds  with  the  greatest  readiness 
upon  platinum  wire  in  the  oxidation  flame  to  a  transparent  bead, 
which  is  yellow  when  hot,  but  colorless  after  being  cooled. 
With  the  addition  of  more  of  the  lead  oxide,  it  becomes  opal 
escent.  When  heated  by  the  intermittent  flame,  and  with  still 
more  of  the  oxide,  it  acquires  a  yellow  enamel  after  cooling. 
Heated  upon  charcoal,  in  the  flame  of  reduction,  the  bead 
spreads  and  becomes  opaque.  After  a  continued  blast,  all 
the  oxide  is  reduced  with  effervescence  to  metallic  lead,  which 
melts  and  runs  towards  the  edges  of  the  bead,  while  the  bead 
again  becomes  transparent. 

Microcosmic  Salt  dissolves  oxides  of  lead  upon  platinum  wire 
in  the  flame  of  oxidation  easily  to  a  clear,  colorless  bead,  which 
appears,  when  highly  saturated,  yellow  while  hot.  A  saturated 
bead  becomes  enamel-like  after  cooling.  The  bead  appears  in 
the  flame  of  reduction,  and  upon  charcoal,  of  a  greyish  color 
and  dull.  By  the  addition  of  more  oxide,  a  yellow  sublimate  of 
protoxide  is  produced  upon  the  charcoal.  By  the  addition  of 
tin,  the  bead  appears  of  a  darker  grey,  but  it  is  never  quite 
opaque. 

Carbonate  of  Soda  dissolves  oxide  of  lead  in  the  flame  of  oxi 
dation  upon  platinum  wire  quite  readily  to  a  transparent  bead, 
which  becomes  yellow  when  cooling,  and  is  opaque.  Upon  char 
coal  in  the  flame  of  reduction,  it  is  rapidly  reduced  to  metallic 


152  THE    BLOWPIPE. 

lead,  which  yields,  after  a  continued  blast,  a  yellow  sublimate 
of  oxide  upon  the  charcoal. 

(b.)  Bismuth  (Bi). — This  metal  occurs  mostly  in  the  metallic 
state,  and  less  frequently  as  the  sulphide.  In  the  pure  metallic 
state,  it  is  of  a  reddish-white  color  and  great  lustre.  It  crys 
tallizes  in  cubes.  It  is  brittle,  and  may  be  readily  pulverize J. 
It  melts  at  476°,  and  is  volatilized  at  a  white  heat.  It  is  solu 
ble  in  nitric  acid,  and  forms  the  nitrate  of  bismuth. 

(a.)  Oxide  of  Bismuth  (Bi2O). — This  oxide  is  a  light  yellow 
powder,  fusible  at  a  red  heat,,  insoluble  in  caustic  potash  and 
ammonia.  It  is  the  base  of  the  salts  of  bismuth.  •  Its  hydrate 
is  white,  and  easily  soluble  in  acids.  The  addition  of  water 
causes  these  solutions  to  become  milky,  because  they  are 
decomposed  into  a  soluble  acidulous  and  an  insoluble  basic 
salt  of  bismuth. 

(j3.)  Peroxide  of  Bismuth  (BiO2)  is  a  dark-colored  powder, 
completely  soluble  in  boiling  nitric  acid,  and  yielding  oxygen  ; 
produces,  with  hydrochloric  acid,  chlorine  gas.  It  can  be 
heated  up  to  the  temperature  of  620°  without  being  decom 
posed  ;  but,  exposed  to  a  temperature  of  630°  it  yields  oxygen. 
Mixed  with  combustible  substances,  it  glows  with  brightness. 

(y.)  Bismuthic  Acid  (Bia06)  is  a  brown  powder  similar  to 
the  peroxide,  but  is  converted  by  boiling  nitric  acid  into  a 
green,  scarcely  soluble  substance  (Bi303,  Bi806).  Its  hydrate 
is  of  a  red  color. 

BLOWPIPE  REACTIONS. — Metallic  bismuth  is  converted,  when 
exposed  upon  platinum  wire  to  the  flame  of  oxidation,  into  a 
dark  brown  oxide,  which  turns  light  yellow  while  cooling.  It 
is  slowly  volatilized  when  heated,  and  a  yellow  sublimate  of 
oxide  is  produced  upon  the  charcoal. 

Oxide  of  bismuth  melts  upon  platinum  foil  in  the  flame  of 
oxidation  very  easily  into  a  dark-brown  liquid,  which  changes 
to  a  light  yellow  while  cooling.  By  too  strong  a  heat,  it  is 
reduced  and  penetrates  the  platinum  foil. 

Upon  charcoal,  in  the  flame  of  oxidation  and  of  reduction,  it  is 
reduced  to  metallic  bismuth,  which  melts  into  one  or  more 


SPECIAL     REACTIONS.  153 

globules.  By  a  continued  blast  they  are  slowly  volatilized,  and 
produce  a  yellow  sublimate  of  oxide  upon  the  charcoal,  beyond 
which  a  white  sublimate  of  carbonate  of  bismuth  is  visible. 
These  sublimates  disappear  in  the  flame  of  reduction,  but  with 
out  communicating  any  color  to  it. 

Borax  dissolves  oxide  of  bismuth  upon  platinum  wire,  in  the 
flame  of  oxidation,  easily  to  a  clear  yellow  bead,  which  appears 
colorless  after  cooling.  By  the  addition  of  more  oxide,  the  hot 
bead  becomes  orange.  It  turns  more  yellow  while  cooling,  and 
when  cool  is  opalescent.  Upon  charcoal  in  the  flame  of  reduc 
tion,  the  bead  becomes  turbid  and  greyish  colored.  The  oxide  is 
reduced  with  intumescence  to  the  metallic  state,  and  the  bead 
becomes  clear  again.  The  addition  of  tin  promotes  the  reduc 
tion. 

Microcosmic  Salt  dissolves  oxide  of  bismuth  upon  platinum 
wire,  in  the  flame  of  oxidation,  to  a  yellow  bead,  which  becomes 
colorless  after  cooling.  By  the  addition  of  more  oxide,  the 
bead  is  yellowish-brown  while  hot,  and  colorless  after  cooling, 
but  not  quite  transparent.  This  bead  becomes  enamelled  when 
heated  by  the  intermittent  flame  ;  also,  by  the  addition  of  still 
more  of  the  oxide,  after  it  is  cooled. 

Upon  charcoal,  in  the  flame  of  reduction,  and  particularly 
with  the  addition  of  tin,  the  bead  is  colorless  and  transparent 
while  hot,  but  while  cooling  becomes  of  a  dark-gray  color  and 
opaque. 

Oxide  of  bismuth  is  reduced,  by  fusion  with  carbonate  of  soda, 
as  well  in  the  oxidating  as  in  the  reducing  flame,  instantly  to 
metallic  bismuth. 

As  the  above  mentioned  higher  oxides  of  bismuth  are  con 
verted  by  ignition  into  oxide  of  the  metal  and  free  oxygen, 
they  have  the  same  behavior  before  the  blowpipe. 

As  bismuth  occurs  mostly  in  the  metallic  form,  it  is  neces 
sary  to  know  how  to  distinguish  it  from  metals  similar  to 
it.  Its  brittleness  distinguishes  it  from  lead,  zinc  and  tin,  as 
they  are  readily  flattened  by  a  stroke  of  the  hammer,  while 
bismuth  is  broken  to  pieces.  Bismuth,  in  this  latter  respect, 

7* 


154  THE     BLOWPIPE. 

might  perhaps  be  mistaken  for  antimony  or  tellurium  ;  but,  by 
the  following  examination,  it  is  easy  to  separate  bismuth  from 
antimony  or  tellurium. 

1.  Neither  bismuth  nor  antimony  sublimates  when  heated  in 
a  glass  tube  closed  at  one  end.     At  a  temperature  which  is 
about  to  fuse  the  glass,  tellurium  yields  a  small  quantity  of  a 
white  vapor  (some  tellurium  is  oxidized  to  tellurous  acid  by 
the  oxygen  of  the  air  in  the  tube).    After  that,  a  grey  metallic 
sublimate  settles  on  the  sides  of  the  tube. 

2.  Heated  in  an  open  tube,  antimony  yields  a  white  vapor, 
which  coats  the  inside  of  the  glass  tube,  and  can  be  driven  by 
heat  from  one  part  of  the  tube  to  another  without  leaving  a 
residue.     The  metallic  globule  is  covered  with  a  considerable 
quantity  of  fused  oxide.     Tellurium  produces,  under  the  same 
circumstances,  an  intense  vapor,  and  deposits  on  the  glass  a 
white   powder,   which  melts  by  heat  into    globules  that  ruu 
over  the  glass.     The  metallic  globules  are  covered   by  fused, 
transparent,  and  nearly  colorless  oxide,  which  becomes  white 
while  cooling.     By  a  high  temperature,  and  with  little  access 
of  air,  metallic  tellurium  sublimes  with  the  deposition  of  a 
grey  powder.     Bismuth   produces,    under   similar   treatment, 
scarcely  any  vapor,  unless  it  is  combined  with  sulphur.     The 
metal   is  enveloped   by  fused  oxide  of  a  dark  yellow  color, 
which  appears  light  yellow  after  being  cooled.     It  acts  upon 
the  glass,  and  dissolves  it. 

3.  Upon  charcoal,  exposed  to  the  blowpipe  flame,  the  three 
metals  are  volatilized,  and  yield  a  sublimate  upon  the  charcoal. 
That  of  antimony  is  white,  while  those  of  bismuth  and  tellurium 
are  dark  yellow.     By  exposing  them  to  the  flame  of  reduction, 
the  sublimate  of  tellurium  disappears  and  communicates  an 
intense  green  color  to  the  flame.     The  antimony  incrustation 
gives  a  feeble  greenish-blue  color,  while  the  sublimate  of  bis 
muth  gives  no  perceptible  color  in  the  light.     It  is,  however, 
worthy  of  notice  that  if  the  operation  takes  place  in  the  dark, 
a  very  pale  blue  flame  will  be  seen  with  the  bismuth. 

(c.)  Tin  (Sn). — This  metal  does  not  occur  in  nature  in  the 


SPECIAL     REACTIONS. 

metallic  state,  very  seldom  in  the  sulphide,  but  chiefly  in  the 
oxide  (tinstone).  In  the  metallic  state  it  is  silver-white,  pos 
sesses  a  very  high  lustre,  is  soft  (but  harder  than  lead),  ductile, 
but  has  not  much  tenacity,  and  it  is  very  malleable.  The 
metal  when  it  is  cast  gives  a  peculiar  creaking  noise  when 
twisted  or  bent,  which  proceeds  from  the  crystalline  structure 
of  the  metal.  This  crystallization  is  quite  clearly  manifested 
by  attacking  the  surface  of  the  metal,  or  that  of  tin  plate, 
with  acids. 

Tin  is  very  slightly  tarnished  by  exposure  to  the  air.  It 
fuses  at  442°,  and  becomes  grey,  being  a  mixture  of  the  oxide 
and  the  metal.  At  a  high  temperature  even,  tin  is  but  little 
subject  to  pass  off  as  vapor.  It  is  soluble  in  aqua  regia,  and 
with  the  liberation  of  hydrogen,  in  hot  sulphuric  and  hydro 
chloric  acids,  and  in  cold  dilute  nitric  acid,  without  decom 
posing  water,  or  the  production  of  a  gas,  while  nitrate  of  tin 
and  nitrate  of  ammonia  are  formed.  Concentrated  nitric  acid 
converts  tin  into  insoluble  tin  acids. 

(a.)  Protoxide  of  Tin  (SnO)  is  a  dark-grey  powder.  Its 
hydrate  is  white,  and  is  soluble  in  caustic  alkalies.  When  this 
solution  is  heated,  anhydrous  crystalline  black  protoxide  is 
separated.  The  soluble  neutral  salts  of  tin-protoxide  are  de 
composed  by  the  addition  of  water,  and  converted  into  acid 
soluble,  and  basic  insoluble  salts. 

When  protoxide  of  tin  is  ignited  with  free  access  of  air,  it 
takes  fire  and  is  converted  with  considerable  intensity  into  the 
acids,  producing  white  vapors.  This  is  likewise  the  case  if  it  is 
touched  by  a  spark  of  fire  from  steel.  The  hydrate  of  the  prot 
oxide  of  tin  can  be  ingnited  by  the  flame  of  a  candle,  and 
glows  like  tinder. 

((3.)  Sesquioxide  of  Tin  (Sna03)  is  a  greyish-brown  powder. 
Its  hydrate  is  white,  with  a  yellow  tinge.  It  is  soluble  in 
aqua  ammonia  and  in  hydrochloric  acid ;  this  solution  forms 
with  solution  of  gold  the  "  purple  of  Cassius." 

(y.)  Stannic  Add  (peroxide,  SnO5). — This  acid  occurs  in  na 
ture  crystallized  in  quadro-octahedrons,  of  a  brown  or  an  intense 


156  T  H  K    BLOWPIPE. 

black  color,  and  of  great  hardness  (tinstone ).  Artificially  pre 
pared,  it  is  a  white  or  yellowish-white  powder.  It  exists  in 
two  distinct  or  isomeric  modifications,  one  of  which  is  insoluble 
in  acids  (natural  tin-acid)  while  the  other  (tin-acid  prepared  in 
the  wet  way)  is  soluble  in  acids.  By  ignition  the  soluble  acid 
is  converted  into  the  insoluble.  Both  modifications  form 
hydrates. 

Reactions  before  the  Blowpipe. — Metallic  tin  melts  easily.  It 
is  covered  in  the  flame  of  oxidation  into  a  yellowish-white 
oxide,  which  is  carried  off  sometimes  by  the  stream  of  air 
which  propels  the  flame.  In  the  reduction  flame,  and  upon 
charcoal,  melting  tin  retains  its  metallic  lustre,  while  a  thin 
sublimate  is  produced  upon  the  charcoal.  This  sublimate  is 
light-yellow  while  hot,  and  gives  a  strong  light  in  the  flame  of 
oxidation,  and  turns  white  while  cooling.  This  sublimate  is 
found  near  to  the  metal,  and  cannot  be  volatilized  in  the  oxida 
tion  flame.  In  the  flame  of  reduction  it  is  reduced  to  metallic 
tin.  Sometimes  this  incrustation  is  so  imperceptible  that  it 
can  scarcely  be  distinguished  from  the  ashes  of  the  charcoal. 
If  such  be  the  case,  moisten  it  with  a  solution  of  cobalt,  and 
expose  it  to  the  flame  of  oxidation,  when  the  sublimate  will 
exhibit,  after  cooling,  a  bluish-green  color. 

Protoxide  of  tin  takes  fire  in  the  flame  of  oxidation,  and 
burns  with  flame  and  some  white  vapor  into  tin  acid,  or  stannic 
acid.  In  a  strong  and  continued  reduction  flame,  it  may  be 
reduced  to  metal,  when  the  same  sublimate  above  mentioned 
is  visible.  The  sesquioxide  of  tin  behaves  as  the  above. 

Stannic  acid,  heated  in  the  flame  of  oxidation,  does  not  melt 
and  is  not  volatilized,  but  produces  a  strong  light,  and  appears 
yellowish  while  hot,  but  changing  as  it  cools  to  a  dirty-yellow 
white  color.  In  a  strong  and  continued  flame  of  reduction,  it 
may  be  reduced  likewise  to  the  metallic  state,  with  the  produc 
tion  of  the  same  sublimate  as  the  above. 

Borax  dissolves  tin  compounds  in  the  flame  of  oxidation,  and 
upon  platinum  wire,  very  tardily,  and  in  small  quantity,  to  a 
transparent  colorless  bead,  which  remains  clear  after  cooling. 


S  v  K  c  i  A  L     REACTIONS.  157 

and  also  when  heated  interrnittingly.  But  if  a  saturated  bead, 
after  being  completely  cool,  is  exposed  again  to  the  flame  of 
oxidation,  at  a  low  red  heat,  the  bead  while  cooling  is 
opaque,  loses  its  globular  form,  and  exhibits  an  indistinct  crys 
tallization.  This  is  the  case  too  in  the  flame  of  reduction,  but 
if  the  bead  is  highly  saturated,  a  part  of  the  oxide  is  reduced. 

Microcosmic  Salt  dissolves  the  oxides  in  the  flame  of  reduc 
tion  very  tardily  in  a  small  quantity  to  a  transparent  colorless 
bead,  which  remains  clear  while  cooling.  If  to  this  bead  ses- 
quioxide  of  iron  is  added  in  proper  proportion,  the  sesquioxide 
loses  its  property  of  coloring  the  bead,  but  of  course  an  excess 
of  the  iron  salt  will  communicate  to  the  bead  its  own  charac 
teristic  color.  In  the  flame  of  reduction  no  further  alteration 
is  visible. 

Tin-oxides  combine  with  carbonate  of  soda,  in  the  flame  of 
oxidation  upon  platinum  wire,  with  intumescence  to  a  bulky 
and  confused  mass,  which  is  insoluble  in  more  soda.  Upon  char 
coal,  in  the  reduction  flame,  it  is  easily  reduced  to  a  metallic 
globule.  Certain  compounds  of  tin-oxides,  particularly  if  they 
contain  tantalum,  are  by  fusion  with  carbonate  of  soda  reduced 
with  difficulty  ;  but  by  the  addition  of  some  borax,  the  reduc 
tion  to  the  metallic  state  is  easily  effected. 

Tin-oxides  exposed  to  the  oxidation  flame,  then  moistened 
with  a  solution  of  cobalt,  and  exposed  again  to  the  flame  of 
oxidation,  will  exhibit,  after  having  completely  cooled,  a  bluish- 
green  color. 


EIGHTH    GROUP. MERCURY,    ARSENIC. 

These  two  metals  are  volatilized  at  a  temperature  lower 
than  that  of  a  red  heat,  and  produce,  therefore,  no  reactions 
with  borax  and  microcosinic  salt.  Their  oxides  are  easily 
reduced  to  the  metallic  state. 

(a.)  Mercury  (Hg). — This  metal  occurs  in  nature  chiefly 
combined  with  sulphur  as  a  bisulphide. 


158  THE     BLOWPIPE. 

It  occurs  still  more  rarely  in  the  metallic  form,  or  combined 
with  silver,  selenium,  or  chlorine. 

Mercury,  in  the  metallic  state,  has  a  strong  lustre,  and  is 
liquid  at  ordinary  temperatures,  whereby  it  is  distinguished 
from  any  other  metal.  It  freezes  at  40°  and  boils  at  620°, 
but  it  evaporates  at  common  temperatures.  Pure  mercury  is 
unalterable.  Upon  being  exposed  to  the  air,  it  tarnishes  only 
by  admixture  with  other  metals,  turns  grey  on  the  surface,  and 
loses  its  lustre.  It  is  soluble  in  cold  nitric  acid  and  in  concen 
trated  hot  sulphuric  acid,  but  n<3t  in  hydrochloric  acid. 

(X-)  Protoxide  of  Mercury  (Hg20). — It  is  a  black  powder, 
which  is  decomposed  by  ignition  into  metallic  mercury  and  oxy 
gen.  By  digestion  with  certain  acids,  and  particularly  with 
caustic  alkalies,  it  is  converted  into  metallic  mercury  and  per 
oxide.  Some  neutral  salts  of  the  protoxide  are  only  partly 
soluble  in  water,  as  they  are  converted  into  basic  insoluble  and 
acid  soluble  salts. 

Protoxide  of  mercury  is  completely  insoluble  in  hydrochloric 
acid.  Its  neutral  salts  change  blue  litmus  paper  to  red. 

(/3.)  Peroxide  of  Mercury  (HgO). — This  oxide  exists  in  two 
allotropic  modifications.  One  is  of  a  brick-red  color,  and  the 
other  is  orange.  Being  exposed  to  heat,  they  turn  black,  but 
regain  their  respective  colors  upon  cooling.  They  are  decom 
posed  at  a  high  temperature  into  metallic  mercury  and  oxygen. 
They  yield  with  acids  their  own  peculiar  salts. 

Mercury,  in  the  metallic  form,  can  never  be  mistaken  for  any 
other  metal  in  consequence  of  its  fluid  condition  at  ordinary 
temperatures. 

Exposed  to  the  blowpipe  flame,  it  is  instantly  volatilized. 
This  is  also  the  case  with  it  when  combined  with  other 
metals.  The  oxides  of  mercury  are,  in  the  oxidation  and 
reduction  flames,  instantly  reduced  and  volatilized.  They  do 
not  produce  any  alteration  with  fluxes,  as  they  are  volatilized 
before  the  bead  melts.  Heated  with  carbonate  of  soda  in  a 
glass  tube  closed  at  one  end,  they  are  reduced  to  metallic  mer 
cury,  which  is  volatilized,  and  condenses  upon  a  cool  portion  of 


SPECIAL     REACTIONS.  159 

the  tube  as  a  grey  powder.  By  cautious  knocking  against  the 
tube,  or  by  rubbing  with  a  glass  rod,  this  sublimate  cau  be 
brought  together  into  one  globule  of  metallic  mercury.  Com 
pounds  of  mercury  can  be  most  completely  reduced  by  a  mix 
ture  of  neutral  oxalate  of  potassa  and  cyanide  of  potassium.  If 
the  substance  under  examination  contains  such  a  small  quan 
tity  of  mercury  that  it  cannot  be  distinguished  by  volatilization, 
a  strip  of  gold  leaf  may  be  attached  to  an  iron  wire,  and  intro 
duced  during  the  experiment  in  the  glass  tube.  The  smallest 
trace  of  mercury  will  whiten  the  gold  leaf  in  spots. 

(b.)  Arsenic  (As). — This  metal  occurs  in  considerable  quan 
tity  in  nature,  chiefly  combined  with  sulphur  or  metals. 

Arsenic,  in  the  metallic  state,  is  of  a  whitish-grey  color,  high 
lustre,  and  is  crystalline,  of  a  foliated  structure,  and  is  so  brittle 
that  it  can  be  pulverized.  It  does  not  melt,  but  is  volatilized 
at  356°.  Its  vapor  has  a  strong  alliaceous  odor.  Arsenic 
sublimes  in  irregular  crystals.  By  exposure  to  the  air  it  soon 
tarnishes,  and  is  coated  black.  Being  mixed  with  nitrate  of 
potassa  and  inflamed,  it  detonates  with  vehemence.  Mixed 
with  carbonate  of  potassa,  it  is  inflamed  by  a  stroke  of  the 
hammer,  and  detonates  violently. 

Heated  in  oxygen  gas,  it  is  inflamed,  and  burns  with  a  pale 
blue  flame  to  arsenious  acid. 

((3.)  Arsenious  Acid  (AsO3). — This  acid  crystallizes  in  octa 
hedrons,  or,  when  fused,  forms  a  colorless  glass,  which  finally 
becomes  opaque  and  enamel-like,  or  forms  a  white  powder.  It 
sublimes  without  change  or  decomposition.  When  heated  for 
a  longer  while  below  the  temperature  of  sublimation,  it  melts 
into  a  transparent,  colorless,  tough  glass.  The  opaque  acid  is 
sparingly  soluble  in  cold  water,  and  still  more  soluble  in  hot 
water.  It  is  converted,  by  continued  boiling,  into  the  transpa 
rent  acid,  which  is  much  more  soluble  in  water.  Arsenious  acid 
is  easily  dissolved  by  caustic  potassa.  It  is  also  soluble  in 
hydrochloric  acid.  This  acid  occurs  associated  with  antimo- 
nious  acid,  protoxide  of  tin,  protoxide  of  lead,  and  oxide  of 


160  THE     BLOWPIPE. 

copper.      It  occurs  likewise  in  very  small  quantity  in  ferrugi 
nous  mineral  springs. 

(y.)  Arsenic  Acid  (AsO5)  is  a  white  mass,  which  readily 
absorbs  moisture  and  dissolves.  It  will  not  volatilize  at  a  low 
red  heat,  nor  will  it  decompose.  Exposed  to  a  strong  heat,  it 
is  decomposed,  yielding  oxygen,  and  passing  into  arsenious 
acid. 

Reactions  before  the  Blowpipe. 

Metallic  arsenic,  heated  in  a  glass  tube  closed  at  one  end, 
yields  a  black  sublimate  of  a  metallic  lustre,  and  at  the  same 
time  gives  out  the  characteristic  alliaceous  odor.  This  is  the 
case  too  with  alloys  of  arsenic,  if  there  is  a  maximum  quantity 
of  arsenic  present. 

When  heated  in  a  glass  tube  open  at  both  ends,  metallic 
arsenic  is  oxidized  to  arsenious  acid,  which  appears  as  a  white 
crystalline  sublimate  on  the  sides  of  the  glass  tube.  This 
deposit  will  occur  at  some  distance  from  the  assay,  in  conse 
quence  of  the  great  volatility  of  the  arsenic.  The  sublimate 
can  be  driven  from  one  place  upon  the  tube  to  another,  by  a 
very  low  heat.  Alloys  of  arsenic  are  converted  into  basic 
arseniates  of  metal  oxides,  while  surplus  arsenic  is  converted 
into  arsenious  acid,  which  sublimes  on  the  tube.  If  too  much 
arsenic  is  used  for  this  experiment,  a  dark-brown  incrustation 
will  sublime  upon  the  sides  of  the  tube  which  will  give  an  alli 
aceous  smell.  If  this  sublimate  should  be  deposited  near  the 
assay,  then  it  resembles  the  white  sublimate  of  arsenious  acid. 

Heated  upon  charcoal,  metallic  arsenic  is  volatilized  before 
it  melts,  and  incrusts  the  charcoal  in  the  flame  of  oxidation  as 
a  white  deposit  of  arsenious  acid.  This  sublimate  appears 
sometimes  of  a  greyish  color,  and  takes  place  at  some  dis 
tance  from  the  assay.  When  heated  slightly  with  the  blow 
pipe  flame,  this  sublimate  is  instantly  driven  away,  and  being 
heated  rapidly  in  the  reduction  flame,  it  disappears  with  a 


S  r  K  c  i  A  L     REACTIONS.  161 

light  blue  tinge,  while  the  usual  alliaceous  or  garlic  smell  may 
be  discerned. 

Arsenious  acid  sublimes  in  both  glass  tubes  very  readily,  as  a 
white  crystalline  sublimate.  These  crystals  appear  to  be  regu 
lar  octahedrons  when  observed  under  the  microscope.  Upon 
charcoal  it  instantly  volatilizes,  and  when  heated,  the  character 
istic  garlic  smell  may  be  observed. 

Arsenic  acid  yields,  heated  strongly  in  a  glass  tube  closed  at 
one  end,  oxygen  and  arsenious  acid,  the  latter  of  which  sub 
limes  in  the  cool  portions  of  the  tube.  Compounds  of  arsenic 
produce,  in  consequence  of  their  volatility,  no  reactions  with 
fluxes.  Being  heated  upon  charcoal  with  carbonate  of  soda, 
they  are  reduced  to  metallic  arsenic  which  may  be  detected  by 
the  alliaceous  odor  peculiar  to  all  the  arsenic  compounds  when 
volatilized. 


NINTH    GROUP. — COPPER,    SILVER,    GOLD. 

These  metals  are  not  volatile,  neither  are  their  oxides.  They 
are  reduced  to  the  metallic  state,  by  fusion  with  carbonate  of 
soda,  when  they  melt  to  a  metallic  grain.  The  oxides  of  silver 
and  gold  are  reduced  per  se  to  the  metallic  state  by  ignition. 
In  the  reduction  of  the  oxides  of  this  group,  no  sublimate  is 
visible  upon  the  charcoal, 

(a.)  Copper  (Cu). — This  metal  occurs  in  the  metallic  state, 
also  as  the  protoxide,  and  as  oxides  combined  with  acids  in 
different  salts  (carbonate  of  copper  as  malachite,  etc.)  The  sul 
phide  of  copper  is  the  principal  ore  of  copper  occurring  in  nature. 
In  the  metallic  state,  copper  is  of  a  red  color,  has  great  lustre 
and  tenacity,  is  ductile  and  malleable,  and  crystallizes  in  octa 
hedrons  and  cubes.  It  melts  at  a  bright  red  heat,  is  more 
difficult  than  silver  to  fuse,  but  fuses  more  readily  than  gold. 
It  absorbs  oxygen  while  melting.  There  arises  from  its  surface 
a  fine  dust  of  metallic  globules,  which  are  covered  with  the 
protoxide.  The  surface  of  the  metal  is  likewise  covered  with 


162  THE     BLOWPIPK. 

the  protoxide.  Copper  exposed  to  moist  air  tarnishes,  and  is 
converted  into  hydratic  carbonate  of  copper.  When  ignited 
in  the  open  air,  it  is  soon  covered  with  the  brownish-red  prot 
oxide. 

(%.)  Protoxide  of  Copper  (Cu'O). — This  oxide  occurs  in 
nature,  crystallized  in  octahedrons  of  a  ruby-red  color,  of  a 
lamellar  structure,  and  transparent.  Artificially  prepared,  it 
forms  a  powder  of  the  same  color.  It  is  decomposed  by  dilute 
acids  into  salts  of  peroxide  and  metal.  It  is  converted  by  igni 
tion,  with  free  access  of  air,  into  peroxide. 

(j3.)  Oxide  of  Copper  (CuO). — This  oxide  is  a  dark-brown 
or  black  powder.  It  is  dissolved  by  acids,  with  a  blue  or 
green-colored  solution.  It  is  soluble  in  aqua  ammonia,  and  the 
solution  is  of  a  dark  blue  color. 

Reactions  before  the  Blowpipe. — Oxide  of  copper  exposed 
upon  platinum  wire  to  the  inmost  flame  (the  blue  flame),  com 
municates  to  the  external  flame  a  green  color.  Heated  upon 
charcoal  in  the  oxidation  flame,  it  melts  to  a  black  ball,  soon 
spreads  over  the  charcoal,  and  is  partially  reduced. 

Exposed  to  the  reduction  flame,  at  a  temperature  which  will 
not  melt  copper,  it  is  reduced  with  a  bright  metallic  lustre,  but 
as  soon  as  the  blast  ceases,  the  surface  of  the  metal  becomes 
oxidized,  and  appears  dark  brown  or  black.  If  the  tempera 
ture  is  continued  still  higher,  it  melts  to  a  metallic  grain. 

Borax  dissolves  the  oxide  of  copper  in  the  flame  of  oxidation 
to  a  clear  green-colored  bead,  even  if  the  quantity  of  oxide  be 
quite  small,  but  by  cooling,  the  bead  becomes  blue.  In  the 
flame  of  reduction  upon  platinum  wire,  the  bead  soon  becomes 
colorless,  but  while  cooling  presents  a  red  color  (protoxide  of 
copper).  This  bead  is  opaque,  but,  if  too  much  of  the  oxide 
is  added,  a  part  of  it  is  reduced  to  metal,  which  is  visible  by 
breaking  the  metallic  grain. 

Upon  charcoal,  the  oxide  is  reduced  to  the  metal,  and  the 
bead  appears  colorless  after  cooling.  With  the  addition  of 
Borne  tin,  the  bead  becomes  brownish-red  and  opaque  after 
cooling. 


SPECIAL     REACTIONS.  163 

Microcosmic  Salt  dissolves  oxide  of  copper  in  the  flame 
of  oxidation  to  a  green  bead,  not  so  intensely  colored  as  the 
borax  bead.  In  the  reduction  flame  the  bead,  if  pretty  well 
saturated,  becomes  dark-green  while  hot,  and  brownish-red 
when  cool,  opaque  and  enamel-like.  If  the  oxide  is  so  little 
that  no  reaction  is  visible,  by  the  addition  of  some  tin,  the 
bead  appears  colorless  while  hot,  and  dark  brownish-red  and 
opaque  when  cold. 

Carbonate  of  Scda  dissolves  oxide  of  copper  in  the  oxidation 
flame  upon  platinum  wire,  to  a  clear,  green  bead,  which  loses 
its  color  when  cooling,  and  becomes  opaque. 

Upon  charcoal,  it  is  reduced  to  the  metal,  the  soda  is  ab 
sorbed  by  the  charcoal,  and  the  metallic  particles  melt  with 
sufficient  heat  to  a  grain. 

(b.)  Silver  (Ag). — This  metal  occurs  in  nature  in  the  me 
tallic  state,  and  in  combination  with  other  metals,  particularly 
with  lead.  It  also  occurs  as  the  sulphide  in  several  mines. 
It  crystallizes  in  cubes  and  octahedrons  ;  is  of  a  pure  white 
color,  great  lustre,  is  very  malleable  and  ductile,  and  is  softer 
than  copper,  but  harder  than  gold.  It  is  not  oxidizable,  neither 
at  common  temperatures  nor  at  those  which  are  considerably 
higher.  It  is  soluble  in  dilute  nitric  acid,  and  in  boiling  con 
centrated  sulphuric  acid. 

(%.)  Protoxide  of  Silver  (Ag20). — It  is  a  black  powder. 
It  is  converted  by  acids  and  ammonia  into  oxide  and  metal. 

(|3.)  Oxide  of  Silver  (AgO). — It  is  a  greyish-brown  or 
black  powder,  and  is  the  base  of  the  silver  salts.  With  aqua 
ammonia,  it  is  converted  into  the  black,  fulminating  silver. 

(7.)  Superoxide  or  Binoxide  of  Silver  (AgO2). — This  oxide 
occurs  in  black  needles  or  octahedral  crystals  of  great  metallic 
lustre.  It  is  dissolved  by  the  oxygen  acids  with  the  disen 
gagement  of  oxygen  gas. 

Behavior  before  the  Blowpipe. — When  exposed  to  the  flames 
of  oxidation  and  reduction,  the  oxides  of  silver  are  instantly 
reduced  to  the  metallic  state. 

Borax  dissolves   silver-oxides   upon  platinum   wire   in   the 


16:1:  THE     BLOWPIPE. 

oxidation  flame  but  partially,  while  the  other  portion  is  re 
duced,  the  bead  appearing  opalescent  after  cooling,  in  corres 
pondence  to  the  degree  of  saturation.  The  bead  becomes  grey 
in  the  flame  of  reduction,  the  reduced  silver  melting  to  a  grain, 
and  the  bead  is  rendered  clear  and  colorless  again. 

Microcosmic  Salt  dissolves  oxides  of  silver  in  the  flame  of 
oxidation  upon  platinum  wire  to  a  transparent  yellowish  bead, 
which  presents,  when  much  of  the  oxide  is  present,  an  opales 
cent  appearance. 

In  the  flame  of  reduction,  the  reaction  is  analogous  to  that 
of  borax. 

By  fusion  with  carbonate  of  soda  in  the  oxidation  and  reduc 
tion  flames,  the  silver  oxides  are  instantly  reduced  to  metallic 
silver,  which  fuses  into  one  or  more  grains. 

(c.)  Gold  (Au). — This  metal  occurs  mostly  in  the  metallic 
state,  but  frequently  mixed  with  ores,  and  with  other  metals. 
Gold  crystallizes  in  cubes  and  octahedrons,  is  of  a  beautiful  yel 
low  color,  great  lustre,  and  is  the  most  malleable  and  ductile 
of  all  the  metals.  It  melts  at  a  higher  temperature  than  cop 
per,  gives  a  green  colored  light  when  fused,  and  contracts 
greatly  when  cooling.  It  does  not  oxidize  at  ordinary  tempe 
ratures,  nor  when  heated  much  above  them.  It  is  soluble  in 
nitro-hydrochloric  acid  (aqua  regia). 

(%.)  Protoxide  of  Gold  (Au20). — This  oxide  is  a  dark  violet 
colored  powder  which  is  converted  by  a  temperature  of  540° 
into  metallic  gold  and  oxygen.  It  is  only  soluble  in  aqua 
regia.  Treated  with  hydrochloric  acid,  it  yields  the  chloride 
of  gold  and  the  metal.  With  aqua  ammonia,  it  yields  the  ful 
minating  gold,  which  is  a  blue  mass  and  very  explosive. 

(%.)  Peroxide  of  Gold  (Au203). — This  oxide  is  an  olive- 
green  or  dark  brown  powder,  containing  variable  quantities  of 
water.  Decomposed  at  530°,  it  yields  metallic  gold  and  oxy 
gen. 

Reactions  before  the  Blowpipe. — Oxides  of  gold  are  reduced, 
in  both  the  oxidation  and  reduction  flames,  to  the  metal,  which 
fuses  to  grains 


SPECIAL     REACTIONS.  165 

Borax  does  not  dissolve  it,  but  it  is  reduced  to  the  metallic 
state  in  this  flux  in  either  flame.  The  reduced  metal  fuses 
upon  charcoal  to  a  grain. 

Microcosmic  Salt  presents  the  same  reactions  as  borax. 

When  fused  with  soda,  upon  charcoal,  the  soda  is  absorbed, 
and  the  gold  remains  as  a  metallic  grain. 


TENTH  GROUP. MOLYBDENUM,  OSMIUM. 

These  metals  are  not  volatile,  and  are  infusible  before  the 
blowpipe;  but  some  of  their  oxides  are  volatile,  and  can  be 
reduced  to  an  infusible  metallic  powder. 

(a.)  Molybdenum  (Mo)  occurs  in  the  metallic  state  ;  also 
combined  with  sulphur,  or  as  molybdic  acid  combined  with 
lead.  It  is  a  white,  brittle  metal,  and  is  unaltered  by  expo 
sure  to  the  air.  When  heated  until  it  begins  to  glow,  it  is 
converted  into  a  brown  oxide.  Heated  at  a  continued  dull  red 
heat,  it  turns  blue.  At  a  higher  temperature,  it  is  oxidized  to 
molybdic  acid,  when  it  glimmers  and  smokes,  and  is  converted 
into  crystallized  molybdic  acid  upon  the  surface. 

(%.)  Protoxide  of  Molybdenum  (MoO). — This  oxide  is  a 
black  powder. 

(%.)  Deut oxide  of  Molybdenum  (MoO2). — This  oxide  is  a 
dark  copper-colored  crystalline  powder. 

Reactions  before  the  Blowpipe. — Metallic  molybdenum,  its 
protoxide  and  binoxide,  are  converted  in  the  oxidation  flame 
into  molybdic  acid.  This  acid  fuses  in  the  flame  of  oxidation 
to  a  brown  liquid,  which  spreads,  volatilizes,  and  sublimes  upon 
the  charcoal  as  a  yellow  powder,  which  appears  crystalline  in 
the  vicinity  of  the  assay.  This  sublimate  becomes  white  after 
cooling.  Beyond  this  sublimate  there  is  visible  a  thin  and  not 
volatile  ore  of  binoxide,  after  cooling;  this  is  of  a  dark  copper- 
red  color,  and  presenting  a  metallic  lustre. 

Heated  in  a  glass  tube,  closed  at  one  end,  it  melts  to  a 
brown  mass,  vaporizes  and  sublimates  to  a  white  powder  upon 
a  cool  portion  of  the  tube,  Immediately  above  the  assay,  yel- 


166  THE     BLOWPIPE. 

low  crystals  are  visible;  these  crystals  are  colorless  after  cool 
ing,  and  the  fused  mass  becomes  light  yellow-colored  and  crys 
talline. 

Upon  platinum  foil,  in  the  flame  of  oxidation,  it  melts  and 
vaporizes,  and  becomes  light  yellow  and  crystalline  after  cool 
ing.  In  the  reduction  flame  it  becomes  blue,  and  brown-colored 
if  the  heat  is  increased. 

Upon  charcoal,  in  the  reduction  flame,  it  is  absorbed  by  the 
charcoal;  and,  with  an  increase  of  the  temperature,  it  is  re 
duced  to  the  metal,  which  remains  as  a  grey  powder  after 
washing  off  the  particles  of  charcoal. 

Borax  dissolves  it,  in  the  oxidation  flame,  upon  platinum 
wire  easily,  and  in  great  quantity,  to  a  clear  yellow,  which 
becomes  colorless  while  cooling.  By  the  addition  of  more  of 
the  molybdenic  acid  the  bead  is  dark  yellow,  or  red  while  hot, 
and  opalescent  when  cold.  In  the  reduction  flame,  the  color 
of  the  bead  is  changed  to  brown  and  transparent.  By  the 
addition  of  more  of  the  acid,  it  becomes  opaque. 

Microcosmic  Salt  dissolves  it  in  the  oxidation  flame,  upon 
platinum  wire,  to  a  clear,  yellowish-green  bead,  which  becomes 
colorless  after  cooling.  In  the  reduction  flame  the  bead  is  very 
dark  and  opaque,  but  becomes  of  a  bright  green  after  cooling. 
This  is  the  case  likewise  upon  charcoal. 

Carbonate  of  Soda  dissolves  it  upon  platinum  wire  in  the 
oxidation  flame  with  intumescence,  to  a  clear  bead,  which 
appears  milk-white  after  cooling.  Upon  charcoal  the  soda  and 
the  molybdic  acid  are  absorbed,  the  latter  is  reduced  to  the 
metallic  state,  the  metal  remaining  as  a  grey  powder  after 
washing  off  the  particles  of  charcoal.  When  molybdic  acid,  or 
any  other  oxide  of  this  metal,  is  exposed  upon  platinum  wire,  or 
with  platinum  tongs,  to  the  point  of  the  blue  flame,  a  yellowish- 
green  color  is  communicated  to  the  external  flame.  If  also  any 
of  the  compounds  of  molybdenum  are  mixed  in  the  form  of.  a 
powder  with  concentrated  sulphuric  acid  and  alcohol,  and  the 
latter  inflamed,  the  flame  of  the  alcohol  appears  colored  green. 

(c.)  Osmium  (Os). — This  metal  occurs  associated  with  pla- 


SPECIAL     REACTIONS.  167 

linura.  It  is  of  a  bluish-grey  color,  and  is  very  brittle. 
Ignited  in  the  open  air,  it  is  oxidized  to  volatile  osmic  acid, 
which  is  possessed  of  a  pungent  smell,  and  affects  the  eyes.  It 
communicates  a  bright  white  color  to  the  flame  of  alcohol. 
Osmium  oxide  (OsOa)  is  converted  in  the  oxidation  flame  to 
osmic  acid,  which  is  volatilized  with  a  peculiar  smell,  leaving  a 
sublimate. 

In  the  reduction  flame  it  is  reduced  to  a  dark-brown  infusible 
metallic  powder.  It  produces  no  reactions  with  fluxes.  Car 
bonate  of  soda  reduces  it  upon  charcoal  to  an  infusible  metallic 
powder,  which  appears,  after  washing  off  the  particles  of  char 
coal,  of  a  dark-brown  color. 


ELEVENTH     GROUP. PLATINUM,     PALLADIUM,     IRIDIUM,     RHODIUM, 

RUTHENIUM. 

These  metals  are  infusible  before  the  blowpipe.  They  are 
not  volatile,  nor  are  they  oxidizable.  Their  oxides  are,  in  both 
flames,  reduced  to  a  metallic  and  infusible  powder.  They  give 
no  reactions  with  fluxes,  but  are  separated  in  the  metallic  form. 
These  metals  are  generally  found  associated  together  in  the 
native  platinum,  also  with  traces  of  copper,  lead,  and  iron. 

The  metal  palladium  is  found  native,  associated  with  iridium 
and  platinum.  This  metal  generally  occurs  in  greatest  quan 
tity  in  Brazil. 

The  metal  rhodium  is  found  along  with  platinum,  but  in  very 
small  quantities. 

Iridium  occurs  in  nature  associated  with  osmium,  gold,  and 
platinum,  in  the  mines  of  Russia.  Its  great  hardness  has  ren 
dered  it  desirable  for  the  points  of  gold  pens.  In  South 
America  this  metal  is  found  native,  associated  with  platinum 
and  osmium.  The  latter  metal,  associated  with  platinum  and 
indium,  has  been  found  in  South  America. 

As  these  metals  will  not  oxidize  or  dissolve,  they  cannot  be 
separated  from  each  other  by  the  blowpipe  with  the  reagents 
peculiar  to  that  species  of  analysis.  It  is  true  that  colors  may 


168  THE     BLOWPIPE. 

be  discerned  in  the  beads,  but  these  tints  proceed  from  the  pre 
sence  of  small  traces  of  copper,  iron,  etc. 

The  ore  of  osmium  and  iridinm  can  be  decomposed,  and  the 
former  recognized  by  its  fetid  odor.  This  metal,  strongly 
ignited  in  a  glass  tube  with  nitrate  of  potash,  is  converted  to 
the  oxide  of  osmium,  which  gives  an  odor  not  unlike  the  chlo 
ride  of  sulphur. 

As  the  metals  of  this  group  are  very  rare  ones,  especially  the 
last  four  ones,  we  shall  not  devote  an  especial  division  to  each 
of  them.  For  a  more  detailed  statement  of  their  reactions,  the 
student  is  referred  to  the  large  works  upon  blowpipe  analysis. 


CLASS  III. 

NON-METALLIC    SUBSTANCES. 

1.  Water— 2.  Nitric  Acid — 3.  Carbon— 4.  Phosphorus— 5.  Sul 
phur —  6.  Boron — 7.  Silicon  —  8.  Chlorine — 9.  Bromine. — 
10.  Iodine — 11.  Fluorine — 12.  Cyanogen — 13.  Seleninm. 

(1.)  Water  (HO). — Pure  distilled  water  is  composed  of 
one  volume  of  oxygen,  and  two  volumes  of  hydrogen  gases  ;  or, 
by  weight,  of  one  part  of  hydrogen  to  eight  parts  of  oxygen 
gases.  Water  is  never  found  pure  in  nature,  but  possessing 
great  solvent  properties,  it  always  is  found  with  variable  pro 
portions  of  those  substances  it  is  most  liable  to  meet  with,  dis 
solved  in  it.  Thus  it  derives  various  designations  depending 
upon  the  nature  of  the  substance  it  may  hold  in  solution, 
as  lime-water,  etc. 

In  taking  cognizance  of  water  in  relation  to  blowpipe  analy 
sts,  we  regard  it  only  as  existing  in  minerals.  The  examination 
for  water  is  generally  performed  thus  :  the  substance  may  be 
placed  in  a  dry  tube,  and  then  submitted  to  heat  over  a  spirit- 
lamp.  If  the  water  exists  in  the  mineral  mechanically  it  will 
soon  be  driven  off,  but  if  it  exists  chemically  combined,  the 
heat  will  fail  to  drive  it  off,  or  if  it  does,  it  will  only  partially 


SPECIAL     REACTIONS.  169 

effect  it.  The  water  will  condense  upon  the  cool  portions  of 
the  tube,  where  it  can  be  readily  discerned.  If  the  water  exists 
chemically  combined,  a  much  stronger  heat  must  be  applied  in 
order  to  separate  it. 

Many  substances  may  be  perhaps  mistaken  for  water  by  the 
beginner,  such  as  the  volatile  acids,  etc. 

(2  )  Nitric  Acid  (NO6). — Nitric  acid  occurs  in  nature  in 
potash  and  soda  saltpetre.  These  salts  are  generally  impure, 
containing  lime,  as  the  sulphate,  carbonate  and  nitrate,  and  also 
iron  in  small  quantity.  The  soda  saltpetre  generally  contains 
a  quantity  of  the  chloride  of  sodium.  The  salts  containing 
nitric  acid  deflagrate  when  heated  on  charcoal.  Substances 
containing  nitric  acid  may  be  heated  in  a  glass  tube  closed  at 
one  end,  by  which  the  characteristic  red  fumes  of  nitrous  acid 
are  eliminated.  If  the  acid  be  in  too  minute  a  quantity  to  be 
thus  distinguished,  a  portion  of  the  substance  may  be  intimately 
mixed  with  some  bisulphate  of  potash,  and  treated  as  above. 
The  sulphuric  acid  of  the  bisulphate  combines  with  the  base, 
and  liberates  the  nitric  acid,  while  the  tube  contains  the  nitrous 
acid  gas. 

The  nitrate  of  potassa,  when  heated  in  a  glass  tube,  fuses  to 
a  clear  glass,  but  gives  off  no  water.  When  fused  on  platinum 
wire,  it  communicates  to  the  external  flame  the  characteristic 
violet  color.  When  fused  and  ignited  on  charcoal,  its  surface 
becomes  frothy,  indicating  the  nitric  acid. 

(3.)  Carbon  (C). — Carbon  is  found  in  nature  in  the  pure 
crystallized  state  as  the  diamond.  It  occurs  likewise  in 
several  allotropic  states  as  graphite,  plumbago,  charcoal, 
anthracite,  etc.  It  exists  in  large  quantities  combined  with 
oxygen  as  carbonic  acid. 

The  diamond,  although  combustible,  requires  too  high  a  he'at 
for  its  combustion  to  enable  us  to  burn  it  with  the  blowpipe. 
When  excluded  from  the  air,  it  may  be  heated  to  whiteness 
without  undergoing  fusion,  but  with  the  free  access  of  air  it 
burns  at  a  temperature  of  703°  C,  and  is  converted  into  car 
bonic  acid.  If  mixed  with  nitre,  the  potassa  retains  the  car- 

8 


170  THE     BLOWPIPE. 

bonic  acid,  and  the  carbon  may  be  thus  easily  estimated.  If  a 
mineral  containing  carbonic  acid  is  heated,  the  gas  escapes 
with  effervescence,  or  a  strong  mineral  acid  as  the  hydrochloric 
will  expel  the  acid  with  the  characteristic  effervescence. 

(4.)  Phosphorus,  Phosphoric  Acid  (PO5). — This  acid  occurs 
in  a  variety  of  minerals,  associated  with  yttria,  copper,  uranium, 
iron,  lead,  manganese,  etc.  Phosphoric  acid  may  be  detected 
in  minerals  by  pursuing  the  following  process:  dip  a  small 
piece  of  the  mineral  in  sulphuric  acid,  and  place  it  in  the  plati 
num  tongs:  this  is  heated  at  the  point  of  the  blue  flame,  when 
the  outer  flame  will  become  colored  of  a  greenish-blue  hue. 
This  color  will  not  be  mistaken  for  those  of  boracic  acid,  cop 
per,  or  baryta.  Some  of  the  phosphoric  minerals,  when  heated 
in  the  inner  flame,  will  color  the  outer  flame  green. 

If  alumina  be  present  with  the  phosphoric  acid,  the  following 
wet  method  should  be  adopted  for  the  detection  of  the  latter: 
the  substance  should  be  powdered  in  the  agate  mortar  with  a 
mixture  of  six  parts  of  soda,  and  one  and  a  half  parts  of  silica. 
The  entire  mass  should  now  be  placed  on  charcoal,  and  melted 
in  the  flame  of  oxidation.  The  residue  should  be  treated  with 
boiling  water,  which  dissolves  the  phosphate  and  the  excess  of 
carbonate  of  soda,  while  the  silicate  of  alumina,  with  some  of 
the  soda,  is  left.  The  clear  liquor  is  now  treated  with  acetic 
acid,  and  heated  over  the  spirit-lamp,  and  a  small  portion  of 
crystallized  nitrate  of  silver  added;  a  lemon-yellow  precipitate 
of  phosphate  of  silver  is  quickly  developed.  Previous  to  the 
addition  of  the  nitrate,  the  liquor  should  be  well  heated;  other 
wise,  a  white  precipitate  of  dipyrophosphate  of  silver  will  be 
produced. 

If  the  examination  be  of  any  of  the  metallic  phosphides,  the 
substances  should  be  powdered  in  the  agate  mortar,  and  fused 
with  nitrate  of  potassa  on  the  platinum  wire;  the  fused  mass 
should  be  treated  with  soda  in  the  same  manner  as  any  sub 
stance  containing  phosphoric  acid.  The  metal  and  the  phos 
phorus  are  oxidized,  while  the  phosphate  of  potassa  is  fused, 
and  the  metallic  oxide  separates. 


SPECIAL     REACTIONS.  171 

(5.)  Sulphur  (S). — Sulphur  is  found  native  in  crystals 
It  is  frequently  found  associated  with  lime,  iron,  silica,  carbon, 
etc.,  and  combined  extensively  with  metals. 

The  principal  acid  of  sulphur  (the  sulphuric,  SO3)  occurs 
combined  with  the  earths,  the  alkalies,  and  the  metallic  oxides. 
Native  sulphur  is  recognized,  when  heated  upon  charcoal, 
by  its  odor  (sulphurous  acid)  and  the  blue  color  of  its  flame. 
The  compounds  of  sulphur  may  be  detected  by  several  methods. 
If  the  substance  is  heated  in  a  glass  tube,  closed  at  one  end, 
the  yellow  sublimate  of  sulphur  will  subside  upon  the  cool  por 
tions  of  the  tube;  if  the  substance  should  also  contain  arsenic, 
the  sublimate  will  present  itself  as  a  light  brown  incrustation, 
consisting  of  the  sulphide  of  arsenic. 

If  the  assay  is  heated  in  the  open  glass  tube,  sulphurous  acid 
will  thus  be  generated;  but,  if  the  gas  is  too  little  to  be  de 
tected  by  the  smell,  a  strip  of  moistened  litmus  paper  will  indi 
cate  the  presence  of  the  acid. 

The  assay  will  give  off  sulphurous  fumes  if  heated  in  the 
flame  of  oxidation. 

If  the  powdered  substance  is  fused  with  two  parts  of  soda, 
and  one  part  of  borax,  upon  charcoal,  the  sulphide  of  sodium 
is  formed.  This  salt,  if  moistened  and  applied  to  a  polished 
silver  surface,  will  blacken  it.  The  borax  serves  no  other  pur 
pose  than  to  prevent  the  absorption  of  the  formed  sulphide  of 
sodium  by  the  charcoal.  As  selenium  will  blacken  silver  in  the 
manner  above  indicated,  the  presence  of  this  substance  should 
be  first  ascertained,  by  heating  the  assay;  when,  if  it  be  pre 
sent,  the  characteristic  horse-radish  odor  will  reveal  the  fact. 

Sulphuric  acid  may  be  detected  by  fusing  the  substance  with 
two  parts  of  soda,  and  one  part  of  borax,  on  charcoal,  in  the 
flame  of  reduction ;  the  mass  must  now  be  wetted  with  water, 
and  placed  in  contact  with  a  surface  of  bright  silver;  when,  if 
sulphuric  acid  be  present,  the  silver  will  become  blackened. 

Or  the  substance  may  be  fused  with  silicate  of  soda  in  the 
flame  of  reduction.  In  this  case,  the  soda  combines  with  a  por 
tion  of  the  sulphuric  acid,  which  is  then  reduced  to  the  sul- 


172  THE     BLOWPIPE. 

pbide,  while  the  bead  becomes  of  an  orange  or  red  color, 
depending  upon  the  amount  of  the  sulphuric  acid  present.  If 
the  assay  should,  however,  be  colored,  then  the  previous  treat 
ment  should  be  resorted  to. 

(6.)  Boron,  Boradc  Add  (BO3). — This  acid  occurs  in  nature 
in  several  minerals  combined  with  various  bases,  such  as  mag 
nesia,  lime,  soda,  alumina,  etc.  Combined  with  water,  this 
acid  exists  in  nature  as  the  native  boracic  acid;  this  acid  gives 
with  test  paper  prepared  from  Brazil  wood,  when  moistened 
with  water,  a  characteristic  reaction,  for  the  paper  becomes 
completely  bleached.  An  alcohol  solution  turns  curcuma  test 
paper  brown.  Heated  on  charcoal,  it  fuses  to  a  clear  bead; 
but,  if  the  sulphate  of  lime  be  present,  the  bead  becomes  opaque 
upon  cooling. 

The  following  reaction  is  a  certain  one:  the  substance  is 
pulverized  and  mixed  with  a  flux  of  four  and  a  half  parts  of 
bisulphate  of  potassa,  and  one  part  of  pulverized  fluoride  of 
calcium.  The  whole  is  made  into  a  paste  with  water,  and  the 
assay  is  placed  on  the  platinum  wire,  and  submitted  to  the 
point  of  the  blue  flame.  While  the  assay  is  melting,  fluoboric 
gas  is  disengaged,  which  tinges  the  outer  flame  green.  If  but 
a  small  portion  of  boracic  acid  is  present,  the  color  will  be  quite 
evanescent. 

(7.)  Silica,  Silicic  Acid  (SiO3).— This  acid  exists  in  the 
greatest  plenty,  forming  no  inconsiderable  portion  of  the  solid 
part  of  this  earth.  It  exists  nearly  pure  in  crystallized  quartz, 
chalcedony,  cornelian,  flint,  etc.,  the  coloring  ingredients  of 
these  minerals  being  generally  iron  or  manganese. 

With  microcosmic  salt,  silica  forms  a  bead  in  the  flame  of  oxi 
dation  which,  while  hot,  is  clear,  while  the  separated  silica 
floats  in  it.  A  platinum  wire  is  generally  used  for  the  purpose, 
the  end  of  it  being  first  dipped  in  the  salt  which  is  fused  into  a 
bead,  after  which  the  silica  must  be  added,  and  then  the  bead 
submitted  to  the  flame  of  oxidation. 

The  silicates  dissolve  in  soda  but  partially,  and  then  with 
effervescence.  If  the  oxygen  of  the  acid  be  twice  that  of 


SPECIAL     REACTIONS.  173 

the  base,  a  clear  bead  will  be  obtained  that  will  retain  its 
transparency  when  cold.  If  the  soda  be  added  in  small  quan 
tity,  the  bead  will  then  be  opaque.  In  the  first  instance,  a 
part  of  the  base  which  separates  is  re-dissolved,  and,  therefore, 
the  transparency  of  the  glass;  but,  if  too  large  a  quantity  of 
the  soda  is  added,  the  separation  of  the  base  is  sufficient  to 
render  the  assay  infusible. 

(8.)  Chlorine  (Cl). — Chlorine  exists  in  nature  always  in 
combination,  as  the  chlorides  of  sodium,  potassium,  calcium, 
ammonium,  magnesia,  silver,  mercury,  lead,  copper,  etc. 

The  chlorine  existing  in  metallic  chlorides  may  be  detected 
as  follows:  the  wet  way  may  be  accomplished  in  the  following 
manner.  If  the  substance  is  insoluble,  it  must  be  melted  with 
soda  to  render  it  soluble;  if  it  be  already  soluble  it  must  be 
dissolved  in  pure  water,  and  nitrate  of  silver  added,  when  the 
one  ten-thousandth  part  of  chlorine  will  manifest  its  presence 
by  imparting  a  milky  hue  to  the  fluid. 

By  the  blowpipe,  chlorine  may  be  detected  in  the  following 
manner:  Oxide  of  copper  is  dissolved  in  microcosmic  salt  on 
the  platinum  wire  in  the  flame  of  oxidation,  and  a  clear  bead  is 
obtained.  The  substance  containing  the  chlorine  is  now  added, 
and  heat  is  applied.  The  assay  will  soon  be  enveloped  by  a 
blue  or  purplish  flame.  As  none  of  the  acids  that  occur  in  the 
mineral  kingdom  give  this  reaction,  chlorine  cannot  be  con 
founded  with  them,  for  those  which  impart  a  color  to  the  flame, 
when  mixed  with  a  copper  salt,  will  not  do  so  when  tested  in 
the  microcosmic  salt  bead  as  above  indicated. 

If  the  assay  is  soluble  in  water,  the  following  method  may 
be  followed:  a  small  quantity  of  sulphate  of  copper  or  iron  is 
dissolved;  a  few  drops  of  the  solution  is  placed  upon  a  bright 
surface  of  silver,  and  the  metallic  chloride  added;  when,  if 
chlorine  is  present,  the  silver  is  blackened.  If  the  chloride  is 
insoluble  in  water,  it  must  be  rendered  soluble  by  fusion  upon 
a  platinum  wire  with  soda,  and  then  treated  as  above.* 

*  Plattncr. 


174:  THE     BLOWPIPE. 

(9.)  Bromine  (Br). — The  bromide  of  magnesium  and  sodium 
exists  in  many  salt  springs,  and  it  is  from  these  that  the  bro 
mine  of  commerce  is  obtained.  The  metallic  bromides  give  the 
same  reactions  on  silver  with  the  microcosmic  bead  and  copper 
salt  as  the  metallic  chlorides.  The  purplish  color  which,  how 
ever,  characterizes  the  chlorides,  is  more  inclined  to  greenish 
with  the  bromides.  If  the  substance  be  placed  in  a  flask  or 
glass  tube,  and  fused  with  bisulphate  of  potassa,  over  the 
spirit-lamp,  sulphurous  gas  and  bromine  will  be  eliminated. 
Bromine  will  be  readily  detected  by  its  yellow  color  and  its 
smell.  Bromine  may  be  readily  detected  by  passing  a  current 
of  chlorine  through  the  fluid,  after  which  ether  is  added  and 
the  whole  is  agitated.  The  ether  rises  to  the  top,  carrying 
with  it  the  bromine  in  solution ;  after  being  withdrawn,  this 
ether  is  mixed  with  potassa,  by  which  the  bromide  and  bromate 
of  potassa  are  formed.  The  solution  is  evaporated  to  dryness, 
the  residue  is  fused  in  a  platinum  vessel,  the  bromate  is  decompos 
ed,  while  the  bromide  remains;  this  must  be  distilled  with  sul 
phuric  acid  and  the  binoxide  of  manganese.  A  red  or  brown 
vapor  will  then  appear,  indicating  the  presence  of  bromine;  this 
vapor  will  color  starch  paste — which  may  be  put  in  the  re 
ceiver  on  purpose — of  a  deep  orange  color. 

If,  to  a  solution  containing  a  bromide,  concentrated  sulphuric 
or  nitric  acid  be  added,  the  bromine  is  liberated  and  colors  the 
solution  yellow  or  red.  The  hypochlorites  act  in  the  same 
manner.  The  bromine  salts  are  coming  into  use  extensively  in 
photography,  in  consequence  of  their  greater  sensitiveness  to 
the  action  of  light  than  the  chlorides  alone. 

(10.)  Iodine  (I). — This  element  occurs  in  salt-springs, 
generally  combined  with  sodium;  it  also  exists  in  rock-salt;  it 
has  likewise  been  found  in  sea-water,  also  in  a  mineral  from 
Mexico,  in  combination  with  silver,  and  in  one  from  Silesia,  in 
combination  with  zinc.  As  sea-water  contains  iodine,  we  would 
consequently  expect  to  find  it  existing  in  the  sea-weeds,  and  it 
\s  generally  from  the  ashes  of  these  that  it  is  obtained  in  com 
merce. 


SPECIAL     REACTIONS.  175 

When  the  metallic  iodides  are  fused  with  the  microcosmic 
salt  and  copper,  as  previously  indicated,  they  impart  a  green 
color  to  the  flame.  This  color  cannot  be  mistaken  for  the 
color  imparted  to  the  flame  by  copper  alone.  When  the 
metallic  iodides  are  fused  in  a  glass  tube,  closed  at  one  end, 
with  the  bisulphate  of  potassa,  the  vapor  of  iodine  is  liberated, 
and  may  be  recognized  by  its  characteristic  color.  Those  min 
eral  waters  containing  iodine  can  be  treated  the  same  as  for 
bromine,  as  previously  indicated,  while  the  violet-colored  vapor 
of  the  iodine  can  be  easily  discerned.  The  nitrate  of  silver  is 
the  best  test  for  iodine,  the  yellow  color  of  the  iodide  of  silver 
being  not  easily  mistaken,  while  its  almost  insolubility  in  am 
monia  will  confirm  its  identity.  The  chloride  of  silver,  on  the 
contrary,  dissolves  in  ammonia  with  the  greatest  facility. 

The  reactions  of  iodine  are  similar  to  those  of  bromine  with 
concentrated  sulphuric  acid  and  binoxide  of  manganese,  and 
with  nitric  acid:  The  iodine  is  released  and,  if  the  quantity  be 
not  too  great,  colors  the  liquid  brown.  If  there  be  a  consider 
able  quantity  of  iodine  present,  it  is  precipitated  as  a  dark 
colored  powder.  Either  of  these,  when  heated,  gives  out  the 
violet-color  of  the  iodine. 

With  starch  paste  free  iodine  combines,  producing  a  deep 
blue  compound.  If,  however,  the  iodine  be  in  very  minute 
quantity,  the  color,  instead  of  being  blue,  will  be  light  violet 
or  rose  color. 

If  to  a  solution  of  the  sulphate  of  copper,  to  which  a  small 
portion  of  sulphurous  acid  has  been  added,  a  liquid  containing 
iodine  and  bromine  is  poured  in,  a  dirty,  white  precipitate  of 
the  subiodide  of  copper  is  produced,  and  the  bromine  remains 
in  the  solution.  The  latter  may  then  be  tested  for  the  bromine 
by  strong  sulphuric  acid. 

(11.)  Fluorine  (Fl). — This  element  exists  combined  with 
sodium,  calcium,  lithium,  aluminium,  magnesium,  yttrium, 
and  cerium.  Fluorine  also  exists  in  the  enamel  of  the  teeth, 
and  in  the  bones  of  some  animals.  This  element  has  a  strong 
affinity  for  hydrogen,  and,  therefore,  we  find  it  frequently  in 


176  THE     BLOWPIPE. 

the  form  of  hydrofluoric  acid.  Brazil-wood  paper  is  the  most 
delicate  test  for  hydrofluoric  acid,  which  it  tinges  of  a  light 
yellow  color.  Phosphoric  acid  likewise  colors  Brazil  paper 
yellow,  but  as  this  acid  is  not  volatile  at  a  heat  sufficient  to 
examine  hydrofluoric  acid,  there  can  be  no  mistake.  If  the 
substance  is  supposed  to  contain  this  acid,  it  should  be  placed 
on  a  slip  of  glass,  and  moistened  with  hydrochloric  acid,  when 
the  test  paper  may  be  applied,  and  the  characteristic  yellow 
color  will  indicate  the  presence  of  the  fluorine. 

As  hydrofluoric  acid  acts  upon  glass,  this  property  may  be 
used  for  its  detection.  The  substance  may  be  put  into  a  glass 
tube,  and  sulphuric  acid  poured  upon  it  in  sufficient  quantity 
to  moisten  it;  a  slight  heat  applied  to  the  tube  will  develop 
the  acid,  which  will  act  upon  the  glass  of  the  tube.  If  the 
acid  is  retained  in  the  mineral  by  a  feeble  affinity,  and 
water  be  present,  a  piece  of  it  may  be  put  in  the  tube  and 
heated,  when  the  acid  gas  will  be  eliminated.  The  test  paper 
will  indicate  its  presence,  even  before  it  has  time  to  act  upon 
the  glass.  If  the  temperature  be  too  high,  fluosilicic  acid  is 
generated,  and  will  form  a  silicious  incrustation  upon  the  cool 
portion  of  the  tube. 

If  the  fluorine  is  too  minute  to  produce  either  of  the  above 
reactions,  then  the  following  process,  recommended  by  Plattner, 
should  be  followed  :  the  assay  should  be  mixed  with  metaphos- 
phate  of  soda,  formed  by  heating  the  microcosmic  salt  to  dull 
redness.  The  mass  must  then  be  placed  in  an  open  glass  tube, 
in  such  a  position  that  there  will  be  an  access  of  hot  air 
from  the  flame.  Thus  aqueous  hydrofluoric  acid  is  formed, 
which  can  be  recognized  by  its  smell  being  more  suffocating 
than  chlorine,  and  also  by  the  etching  produced  by  the  conden 
sation  of  vapor  in  the  tube.  Moist  Brazil  paper,  applied  to 
the  extremity  of  the  tube,  will  be  instantly  colored  yellow. 

Merlet's  method  for  the  detection  of  this  acid  is  the  follow 
ing  :  *  Pulverize  the  substance  for  examination,  then  triturate 

*  Quoted  by  Plattner. 


SPECIAL     REACTIONS.  177 

it  to  an  impalpable  powder,  and  mix  it  with  an  equal  part  of 
bisulphate  of  potassa.  Heat  the  mass  gradually  in  a  moderately 
wide  test-tube.  The  judicious  application  of  heat  must  be 
strictly  observed,  for  if  the  operator  first  heats  the  part  of  the 
tube  where  the  assay  rests,  the  whole  may  be  lost  on  account 
of  the  glass  being  shattered.  The  spirit-flame  must  be  first 
applied  to  the  fore  part  of  the  tube,  and  then  made  to  recede 
slowly  until  it  fuses  the  assay.  After  the  mixture  has  been  for 
some  time  kept  in  a  molten  state,  the  lamp  must  be  withdrawn, 
and  the  part  containing  the  assay  severed  with  a  file.  The  fore 
part  of  the  tube  must  then  be  well  washed,  and  afterwards 
dried  with  bibulous  paper.  Should  the  fluorine  contained  in 
the  substance  be  appreciable,  the  glass  tube,  when  held  up  to 
the  light,  will  be  found  to  have  lost  its  transparency,  and  to  be 
very  rough  to  the  touch. 

Great  care  should  be  observed  not  to  allow  this  very  corrosive 
acid  to  come  into  contact  with  the  skin,  as  an  ulcer  will  be  the 
consequence  that  will  be  extremely  difficult  to  heal. 

When  hydrofluoric  acid  comes  in  contact  with  any  silicious 
substance,  hydrofluosilicic  acid  gas  is  always  formed. 

(12.)  Selenium  (Se). — This  element  occurs  in  combination 
with  lead  as  the  selenide,  and  with  copper  as  the  selenide  of 
copper.  It  exists  also  combined  with  cobalt  and  lead,  as  the 
selenide  of  these  metals  ;  also  as  the  selenide  of  lead  and 
mercury. 

The  smallest  trace  of  selenium  may  be  detected  by  igniting 
a  small  piece  of  charcoal  in  the  flame  of  oxidation,  when  the 
peculiar  and  unmistakable  odor  of  decayed  horse-radish  will 
indicate  the  presence  of  "that  element.  An  orange  vapor  is 
eliminated  if  the  selenium  be  present  in  any  quantity,  while ' 
there  is  an  incrustation  around  the  assay  of  a  grey  color,  with 
a  metallic  lustre.  This  incrustation  frequently  presents  a  red 
dish-violet  color  at  its  exterior  edges,  often  running  into  a  deep 
blue.  If  a  substance  containing  selenium  be  placed  in  a  glass 
tube,  closed  at  one  end,  and  submitted  to  heat,  the  selenium  is 
sublimed,  with  an  orange-colored  vapor,  and  with  the  charac- 

8* 


178  THE     BLOW  PIPE. 

teristic  odor  of  that  substance.  Upon  the  cool  portions  of  the 
tube  a  steel-grey  sublimate  is  deposited,  and,  beyond  that,  can 
be  discerned  small  crystals  of  selenic  acid.  If  the  mineral  be 
the  seleniferous  lead  glance,  sulphurous  acid  gas  will  be  given 
off,  and  may  be  detected  by  the  smell,  or  by  a  strip  of  moist 
ened  litmus  paper. 

If  arsenic  is  present,  heating  upon  charcoal  will  quickly  lead 
to  the  determination  of  the  one  from  the  other. 


TABULAR  STATEMENT  OF  THE  REACTION'S  OF  MINERALS  BEFORE  THE 
BLOWPIPE. 

In  PART  THIRD  of  this  work,  commencing  at  page  109,  the 
student  will  find  a  sufficiently  explicit  description  of  the  blow 
pipe  reactions  of  those  principal  substances  that  would  be 
likely  to  come  beneath  his  attention.  The  following  tabular 
statement  of  those  reactions — which  we  take  from  Scheerer 
and  Blanford's  excellent  little  work  upon  the  blowpipe — will  be 
/  of  great  benefit,  as  a  vehicle  for  consultation,  when  the  want 
of  time — or  during  the  hurry  of  an  examination — precludes  the 
attentive  perusal  of  the  more  lengthy  descriptions  in  the  text. 

In  the  examination  of  minerals,  before  the  student  avails 
himself  of  the  aid  of  the  blowpipe,  he  should  not  neglect  to 
examine  the  specimen  rigidly  in  relation  to  its  physical  charac 
ters,  such  as  its  hardness,  lustre,  color,  and  peculiar  crystalliza 
tion.  It  is  where  the  difference  of  two  minerals  cannot  be 
distinguished  by  their  physical  appearance,  that  the  aid  of  the 
blowpipe  comes  in  most  significantly  as  an  auxiliary.  For 
instance,  the  two  minerals  molybdenite  and  graphite  resemble 
each  other  very  closely,  when  examined  in  regard  to  their 
physical  appearance,  but  the  blowpipe  will  quickly  discriminate 
them,  for  if  a  small  piece  of  the  former  mineral  be  placed  in 
the  flame  of  oxidation,  a  bright  green  color  will  be  communi 
cated  to  the  flame  beyond  it,  while  in  the  latter  there  will  be 
no  color.  Thus,  in  a  very  short  time,  these  two  minerals  can 


SPECIAL     EEACTIONS.  1Y9 

be  distinguished  from  each  other  by  aid  of  the  blowpipe,  while 
no  amount  of  physical  examination  could  determine  that  point. 
The  blowpipe  is  equally  an  indispensable  instrument  in  the 
determination  of  certain  minerals  which  may  exist  in  others  as 
essential  or  non-essential  constituents  of  them.  For  instance, 
should  a  minute  quantity  of  manganese  be  present  in  a  mineral, 
it  must  be  fused  with  twice  its  bulk  of  a  mixture  of  two  parts 
of  carbonate  of  soda,  and  one  part  of  the  nitrate  of  potassa,  in 
the  flame  of  oxidation  upon  platinum  foil.  The  manganate  of 
soda  thus  formed  will  color  the  fused  mass  of  a  bluish-green 
tint. 

Or  a  slight  quantity  of  arsenic  may  be  discerned  by  the  fol 
lowing  process  recommended  by  Plattner  :  *  one  grain  of  the 
finely  pulverized  metal  is  mixed  with  six  grains  of  nitrate  of 
potassa,  and  slowly  heated  on  the  platinum  spoon.  By  this 
means  the  metals  are  oxidized,  while  the  arseniate  of  potassa  is 
obtained.  Then  boil  the  fused  mass  in  a  small  quantity  of 
water  in  a  porcelain  vessel  till  all  the  arseniate  is  dissolved. 
The  metallic  oxides  are  allowed  to  subside,  and  the  above 
solution  decanted  off  into  another  porcelain  vessel.  A  few 
drops  of  sulphuric  acid  are  added,  and  the  solution  boiled  to 
expel  the  nitric  acid,  after  which  it  is  evaporated  to  dryness. 
In  this  operation,  the  sulphuric  acid  should  be  added  only  in 
sufficient  quantity  to  drive  off  the  nitric  acid,  or,  at  the  utmost, 
to  form  a  bisulphate  with  the  excess  of  potassa.  When  dry, 
the  salt  thus  obtained  is  pulverized  in  an  agate  mortar,  and 
mixed  with  about  three  times  its  volume  of  oxalate  of  potassa, 
and  a  little  charcoal  powder.  The  mixture  is  introduced  into 
a  glass  bulb  having  a  narrow  neck,  and  gently  warmed  over  a 
spirit-lamp  in  order  to  drive  off  the  moisture,  which  must  be 
absorbed  by  a  piece  of  blotting-paper  in  the  neck  of  the  bulb. 
After  a  short  time,  the  temperature  is  increased  to  a  low  red 
heat,  at  which  the  arsenious  acid  is  reduced  and  the  metallic 
arsenic  sublimed,  and  which  re-condenses  in  the  neck  of  the 

*  Quoted  by  Scheerer. 


180          BEHAVIOR    OF    MINERALS. 

bulb.  If  there  the  arsenic  be  so  small  in  quantity  as  to  exhibit 
no  metallic  lustre,  the  neck  of  the  bulb  may  be  cut  off  with  a 
file  immediately  above  the  sublimate,  and  the  latter  exposed  to 
the  flame  of  the  blowpipe,  when  the  arsenic  is  volatilized,  and 
may  be  recognized  by  its  garlic  odor. 

If  the  presence  of  cadmium  is  suspected  in  zinc-blende,  it  may 
be  detected  by  fusing  a  small  piece  of  the  blende  upon  charcoal 
in  carbonate  of  soda.  The  peculiar  bright  yellow  sublimate  of 
the  oxide  of  cadmium,  if  it  be  present,  will  not  fail  to  indicate 
it.  This  incrustation  can  be  easily  distinguished  from  that  of 
zinc.  Thus,  with  the  three  illustrations  we  have  given,  the 
student  will  readily  comprehend  the  great  utility  of  the  blow 
pipe  in  the  examination  of  minerals. 

Although  the  following  tables  were  not  arranged  especially 
for  the  last  part  of  this  work,  still  this  arrangement  is  so  good 
that  by  their  consultation  the  student  will  readily  comprehend 
at  a  glance  what  requires  some  detail  to  explain,  and  we  feel 
no  hesitation  in  saying  that,  although  they  are  not  very  copi 
ous,  they  will  not  fail  to  impart  a  vast  amount  of  information, 
if  consulted  with  any  degree  of  carefulness. 

The  minerals  given  are  such  as  are  best  known  to  English 
and  American  mineralogists  under  the  names  specified.  For 
more  detailed  reactions  than  could  be  crowded  into  a  table,  the 
student  will  have  to  consult  the  particular  substance  as  treated 
in  Part  Third.  If  this  part  is  perused  carefully  previous  to 
consulting  the  tables,  these  will  be  found  eminently  serviceable 
as  a  refresher  of  the  memory,  and  may  thus  save  much  time 
and  trouble. 

And,  finally,  we  would  certainly  recommend  the  student, 
after  he  shall  have  gone  through  our  little  volume  (if  he  is 
ambitious  of  making  himself  a  thorough  blowpipe  analyst),  to 
then  take  up  the  larger  works  of  Berzelius  and  Plattner,  for 
our  treatise  pretends  to  nothing  more  than  a  humble  intro 
duction  to  these  more  copious  and  scientific  works. 


BEFORE    THE     BLOWPIPE. 


181 


Mineral. 


Formula. 


Behavior 


in  glass-bulb.  on  platinum  foil. 


Diamond  . . 


Graphite. . . 


Anthracite . . . 


Wallsend-coal 


C  with  some 
iron,  silica,  etc. 


C  +  xfl 

and  some  ash. 


C,H,N,0,S 
and  ash. 


Cannel-coal , . 


Brown-coal  . . 


Asphaltum . . . 


C,H,N,0,S 

and  ash. 


C,H,N,0,S 

and  ash. 


C-f  H-J-0. 


Generally  gives  off 
water. 


Evolves  water. 


Intumesces  and 
gives  off  water  and 
tarry  matters  which 
partly  condense  in 
bulb,  and  leave  a 
porous  coke. 


As  the    preceding, 

but  gives  off  more 

tar. 


Gives  off  much 
water  and  tar,  and 
leaves  a  porous  cin 
der  retaining  the 
form  of  the  original 
fragment. 

Fuses  with   ease 
affording   an 


In  fine  powder  is 

slowly  consumed 

without   residue  in 

a  strong   oxidizing 

flame. 

Is  slowly  consumed 

leaving    more   or 

less  ash,  principally 

Fe'O3. 

Is  slowly  consumed 

with  the  exception 

of  a  small  quantity 

of  ash. 

Takes  fire  under 
Blowpipe  flame,  and 
burns  with  a  smoky 
flame,  depositing 
much  soot  and  leav 
ing  a  porous  cinder 
which  burns  slowly 
and  leaves  a  small 
ash. 

Similar  to  the  pre 
ceding.     If  held  to 

the    lamp-flame, 
takes  fire  and  burns 

for  some  seconds. 

Burns    slowly    and 
without  flame,  leav 
ing  some  ash. 


Takes   fire   and 
burns  with  a  bright 


182  BEHAVIOR    OF    MINERALS 

Continuation  of  page  181. 


Mineral. 


Formula. 


Behavior 


in  glass-bulb. 


on  platinum  foil. 


Asphaltum 


C  +  H  +  0. 


ELitcrite  . 


C  +  H. 


Hachettine 


Ozokerite . . 


Amber. 


C  +  H. 


C  +  H. 


C  +  H  +  0. 


empyreumatic  oil 
having  an  alkaline 
reaction,  and  com 
bustible  gases,  and 
leaves  a  carbona 
ceous  residue, 

which  is   entirely 
consumed  under  the 
blowpipe  flame,  ex 
cept  a  little  ash. 

Fuses  and  gives  off 
water  having  an 
acid  reaction,  naph 
tha  and  a  tarry 
fluid,  which  chiefly 
condense  in  the 
neck  of  the  bulb, 
and  leave  a  light, 
pulverulent,  carbo 
naceous  residue. 

Fuses  to  a  clear  co 
lorless  liquid,  which 
solidifies  on  cooling 
and  has  a  tallow- 
like  smell. 

Fuses  readily  to  a 
clear    brown    oily 
fluid,  which   solidi 
fies  on  cooling. 

Fuses  with  diffi 
culty,  and  affords 
water,  an  empyreu 
matic  oil,  and  suc- 
cinic  acid  which 
condense  in  the 


flame   and  a  thick 
smoke. 


Fuses,  takes  fire, 
and  burns  with  a 
smoky  flame,  leav 
ing  a  carbonaceous 
residue,  which  un 
der  the  blowpipe 

flame,  is  quickly 

consumed,  with  the 

exception    of    the 

ashes. 

Fuses,  takes  fire, 
and  burns  with  a 
bright  flame  until 
entirely  consumed. 


As  the  preceding. 


Takes  fire  and  burns 
with  a  yellow  flame 
and  a  peculiar  aro 
matic  odor. 


BEFOKE    THE     BLOWPIPE.  183 

Continuation  of  page  182. 


\TinpraT 

B  e  h  a 

v  i  o  r 

in  glass-bulb. 

on  platinum  foil. 

Amber 

C-f  H-f-0 

neck  of  the   bulb 

Mellite  .  . 

£  liF-f-^S 

leaving    a    shining 
black  residue. 

Gives  off  water     If 

On  charcoal  burns 

heated  to  redness, 
is   carbonized,   and 
gives  a  slight  em- 
pyreumatic  odor. 

to  a  white  ash,  which 
moistened  with  ni 
trate  of  cobalt  and 
heated    shows    the 
alumina  reaction. 

184 


BEHAVIOR    OF    MINERALS 

POTASH. 


I 

>  e  h  a  v  i  o  ] 

r 

,,.         , 

i?         i 

Mineral. 

Jb  o  nun  la. 

(1) 

(2) 

(3) 

in  glass-bulb. 

in  open  tube. 

on  charcoal. 

Nitre  

iff 

Fuses  readily 

Deflagrates 

to  a  clear  li 

leaving  a  sa 

quid  and  with 

line   mass, 

a  strong  heat 

which   is   ab 

boils  with  the 

sorbed   into 

evolution  of 

charcoal   and 

oxygen. 

gives    a    sul 

phur  reaction 

on  silver. 

Polyhalite  

tS  +  lfiTgS 

Gives  off 



Fuses  to  a  red 

i   2(5a°S  -1-  2H 

water. 

dish  bead, 

which  in  the 

reducing  flame 

solidifies   and 

shrinks    to    a 

hollow  crust. 

BEFORE    THE     BLOWPIPE.  185 

Continuation  of  page  184. 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

CO 
with  carb.  soda. 

On  platinum 

__ 

__ 



With  bisul- 

wire  fuses  and 

phate  of  pot- 

colors  the 

assa  in  the 

flame  violet 

glass-bulb 

more  or  less 

evolves 

modified  by 

nitrous  fumes. 

lime  and  soda. 

On  platinum 

Dissolves  with 

As  in  borax. 

Fuses.     The 

The  alkaline 

wire  fuses  and 

ebullition  to  a 

alkalies   are 

mass  when 

colors  the 

clear  glass, 

absorbed  by 

laid  on  silver 

flame  yellow 

which  is 

the  charcoal 

gives  a  sul 

from  a  small 
quantity  of 
soda. 

slightly  co 
lored  by  iron, 
and  when  sa 

leaving  the 
lime  and  mag 
nesia  infusible 

phur  reaction. 

turated    be 

on  the  surface. 

comes  opaque 

on  cooling. 

186  BEHAVIOR    OF    MINERALS 

SODA. 


Mineral. 

lTfYi*T¥in1a 

] 

3  e  h  a  v  i  o 

r 

.T  U  1  IIlUl(i. 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

Rock-salt  

NaCl. 

Fuses  to  a 

Fuses    is   ab 

clear  liquid. 

sorbed  by  the 

charcoal   and 

partially  vola 

tilized  incrust- 

ing  the  char 

coal  around. 

Natron  ... 

NaC-flofl: 

Fuses  with 

Fuses    and  is 

the  evolution 

absorbed  into 

X 

of  water. 

the  pores  of 

the  charcoal. 

Soda-nitre  .... 

*Ta£ 

Fuses,  and  if 

Deflagrates 

strongly  heat 

and  is  ab 

ed  evolves  ni 

sorbed  into 

trous  fumes. 

the  charcoal. 

Glauber-salt..  . 

ftaS-f-loB 

Fuses  and 

Fuses,  and  is 

gives  off  water 

absorbed  by 

having  a  neu 

the  charcoal. 

tral  reaction. 

The  saturated 

charcoal   laid 

upon  silver 

gives  the  sul 

phur  reaction. 

Glauberite  .... 

frag  -}-  Ga'S. 

Decrepitates 

Fuses  to  a 

with  the  evo 

clear  bead, 

lution  of  more 

then    spreads 

or  less  water, 

out  ;  the  soda 

and  when 

is   absorbed 

strongly  heat 

and  the  lime 

ed  fuses  to  a 

left  on  the 

clear   liquid. 

surface.   Laid 

on  silver,  the 

fused  mass 

gives   a   sul 

phur  reaction. 

BEFORE    THE     BLOWPIPE.  187 

SODA.     (Continuation  of  page  186.) 


Behavior 

(8) 

C*~  ,,  rt:~i 

(4) 

(5) 

(6) 

cn 

opecial 
reactions. 

in  forceps. 

in  borax. 

in  mic.  salt. 

with  carb.  soda. 

Fuses  with 

_ 

_ 

Gives  the 

great  ease  and 

chlorine  reac 

colors  the 

tions. 

flame  yellow. 

Fuses  and  be 

Dissolves  in 

haves  as  the 

acids  with 

preceding. 

violent  effer 

vescence. 

Deflagrates  on 





_ 

In  a  glass-bulb 

platinum  wire, 

with  bisul- 

coloring   the 
flame  yellow. 

phate  of  pot- 
assa,  gives  the 

NOB-reaction. 

Fuses  and  co 

_ 



__ 

Gives  the 

lors  the  flame 

S03-reaction. 

yellow. 

Fuses  easily 

Fuses  easily 

As  in  borax. 

As   alone  on 

As  in  the  pre 

to  a  clear 

and  gives  the 

charcoal. 

ceding. 

glass,  color 

lime  reaction. 

ing  the  flame 

yellow. 

188  BEHAVIOR     OF     MINERALS 

SODA.     (Continuation  of  page  187.) 


I 

t  e  h  a  v  i  o  i 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(8) 

on  charcoal. 

fraB2-f-10fi 

Intumesces 

Cryolite. 

SNaFl  -f-  Al2Fla 

with  the  evo 
lution  of  wa 
ter,  and  under 
a  strong  heat 
fuses. 

If  heated  so 

and  fuses  to  a 
clear  bead 
more  or  less 
colored   by 
impurities. 

Fuses  to  a  lim 

slightly  and 
gives  a  trace 
of  water. 

that  the  flame 
be  allowed  to 
play  up  the 
tube  upon  the 
mineral,  fluo 
rine  is  evolv 
ed,  which  cor 
rodes  the  in 
terior  of  the 
tube. 

pid  bead,  which 
on  cooling  be 
comes  a  white 
enamel.     If 
heated  for 
some  time,  it 
bubbles,  gives 
off  fluorine 
and  becomes 
infusible. 

BEFORE    THE     BLOWPIPE.  189 

SODA.     (Continuation  of  page  188.) 


Behavior 

(8) 

(4) 

(5) 

(6) 

CO 

Special 
reactions. 

in  forceps. 

in  borax. 

in  mic.  salt. 

with  carb.  soda. 

As  on  char 

Fuses  to  a 

Gives  the 

coal. 

clear  bead, 

boracic-acid- 

which   be 

reaction. 

comes  crys 

talline  on 

cooling. 

Fuses,  color 

Dissolves  to  a 

As  in  borax. 

Fuses  to  a 

If  the  alumina 

ing  the  flame 

clear  bead, 

clear  bead, 

residue  ob 

yellow. 

which  is  ren 

then  spreads 

tained  be 

dered  opaque 

out   on   the 

moistened  with 

by  a  large 

charcoal,  the 

cobalt  solution 

addition. 

soda   is    ab 

and  heated 

sorbed,  and  an 

strongly,  it 

infusible  mass 

assumes   a 

of  alumina 

beautiful  blue 

remains. 

color. 

190  BEHAVIOR     OF     MINERALS 

BARYTA      AND      STRONTIA. 


Mineral. 

Formula. 

Behavior 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

Heavy-spar  .  .  . 

BaS. 

Sometimes 
decrepitates 
and  gives  off 
more    or  less 
water. 

Fuses   in   the 
reducing 
name. 

Celestine  

SrS. 

— 

— 

Fuses  to  a 
milk-white 
bead. 

Witherite  

Bad 

Decrepitates 
more  or  less 
and  evolves 
water. 

~~~ 

Fuses,    effer 
vesces,  and  is 
partially  ab 
sorbed  by  the 
charcoal 

Strontianite  ..  . 

SrC. 

Becomes 
opaque. 

As  in  the  for 
ceps. 

Barytocalcite.  . 

BaC  +  CaC. 

As   the  pre 
ceding. 

— 

In  powder 
frits  together, 
but  does  not 
fuse. 

B  E  F  U  It  E      THE       BLOWPIPE.  191 

BARYTA   AND    STRONTIA.     (Continuation  of  page  190.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

(7) 
with  carb.  soda. 

Fuses  with 

Gives  the 

As  in  borax. 

Fuses  to  a 

If  fused  with 

difficulty  on 

baryta-reac 

clear  bead  ; 

potassa  on  pla 

edges.    Colors 

tion. 

then    spreads 

tinum,  gives 

the  outer  flame 

out  and  is  ab 

the  S03-reac- 

green.    In  the 

sorbed   into 

tion. 

reducing  flame 

the   charcoal. 

forms  BaS, 

The   fused 

which  fuses 

mass  laid  on 

readily. 

silver,    gives 

the  S-reac- 

tion. 

Colors  the 

Gives  the 

As  in  borax. 

Similar  to  the 

Similar  to  the 

flame  crimson. 

strontia-reac- 

preceding. 

preceding. 

tion. 

Colors  the 

Dissolves  with 

As  in  borax. 

Fuses  to  a 

In  dilute  HC1 

outer  flame 

effervescence 

clear  bead  ; 

dissolves  with 

intensely 

and  gives  the 

then  spreads 

much   effer 

green. 

baryta-reac 

out  and  passes 

vescence. 

tion. 

into  the  char 

coal. 

Exfoliates 

Resembles  the 

As  in  borax. 

As   the   pre 

As  the   pre 

and  becomes 

preceding. 

ceding. 

ceding. 

arborescent. 

The  filaments 

glow  brilliantly 

« 

and  fuse  on  the 

point.    Colors 

the  flame  bril 

liantly  crim 

son. 

Colors  the 

Dissolves  with 

As  in  borax, 

Fuses,  and  is 

As  witherite. 

Maine  green  in 

effervescence. 

but  the  satu 

partially  ab 

the  centre  and 
red  towards 

In  large  quan 
tity   gives   a 

rated  bead  is 
milk-white. 

sorbed  leaving 
the   lime   on 

the    point. 

semi-crystal 

the  surface. 

line  bead. 

192  BEHAVIOR    OF     MINERALS 

LIME. 


Mineral 

] 

3  e  h  a  v  i  o 

r 

£  oriiiuni. 

CD 

(2) 

(3) 

in  glass-bulb. 

in  open  tube. 

on  charcoal. 

Gypsum  . 

CaS  +  2fi. 

Turns  white 

In  the  reducin- 

giving  off  wa 

flame  forms 

ter  and  being 

CaS,  which  has 

converted  into 

an  alkaline  re 

plaster  of 

action  on  test 

Paris. 

paper,   and 

gives   a   sul 

phur-reaction 

when  laid  on 

silver  and 

moistened. 

Apatite      .... 

Ca  J  C14-3Ca3I5 

Occasionally 

\ja,f.         —f-wa  J. 

decrepitates 

and  gives  off 

some  water. 

Pharmacolite  .  . 

6a,lg  +  6a 

Gives  off  wa 

Fuses  to  an 

ter,  and  emits 

opaque   bead 

an   arsenical 

and   emits  a 

odor. 

strong  smell 

> 

of  arsenic. 

Cafl 

Turns  white 

Turns  white, 

and  sometimes 

or  brown   if 

decrepitates- 

containing 

Strongly  heat 

much  iron  or 

ed   loses  CO2 

manganese, 

and   becomes 

and  glows 

caustic. 

brilliantly. 

BEFORE     THE     BLOWPIPE. 
LIME.     (Continuation  of  page  192.) 


193 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

cn 

with  carb.  soda. 

Fuses  with 

Dissolves  to  a 

As  in  borax. 

Behaves  as 

Gives  the 

difficulty  to  a 

clear  bead, 

lime.      The 

sulphuric- 

bead,  coloring 

which  gives 

alkaline  mass 

acid-reaction. 

the  flame  red. 

the  lime-reac 

laid  on  silver 

tion. 

and  moistened 

gives  the  sul 

phur-reaction. 

IV. 

Dissolves  easily 

Gives  the 

Is  infusible. 

With  micro- 

Previously 

and  when   in 

lime-reaction. 

The  alkali  is 

cosmic  salt  and 

dipped  in  SO3 

some  quantity 

absorbed,  leav 

oxide  of  cop 

colors  the 

gives  an  opa 

ing   the   lime 

per,  gives  the 

flame  green, 

line   bead. 

\ 

on  the  surface 

chlorine-reac 

afterwards 

of  the  char 

tion.      With 

red. 

coal. 

microcosmic 

salt  in  the  open 

tube  evolves 

fluorine. 

Fuses  to  a 

Dissolves 

As  in  borax. 

Fuses,  and 

translucent 

readily  to  a 

emits  As.  The 

violet  colored 

bead  strongly 

alkali  is  then 

bead,  the  color 

colored  by 

absorbed  by 

being  due  to 

cobalt,  which 

the  charcoal, 

cobalt    Colors 

obscures    the 

as  in  the  pre 

the  flame  blue 

lime-reaction. 

ceding. 

at  first,  then 

faintly  red. 

Glows  bril 

Dissolves  with 

As  in  borax. 

Fuses,  and  be 

Dissolves  with 

liantly,  color 

evolution  of 

haves  as  other 

effervescence 

ing  the  flame 

CO2  and  when 

lime-salts. 

in  cold  HC1. 

red.  Becomes 
caustic    and 

pure  gives  the 
lime-  reaction. 

shows  a  strong 

The    bead    is 

alkaline  reac 

generally  more 

tion. 

or  less  colored 

by   iron   and 

manganese. 

194 


BEHAVIOR    OF    MINERALS 

LIME.     (Continuation  of  page  193.) 


I 

1  e  h  a  v  i  o  i 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

Fluorspar  

CaFl. 

Phosphoresces 

Fuses  easily  to 

with  various 
colors,  when 
heated  in  the 
dark.     Some 
times   decre 
pitates   and 
gives  a  trace 
of  water.   Be 
comes  opales 
cent. 

a  clear  bead, 
which  becomes 
opaque  on 
cooling,  then 
loses  fluorine, 
glows    brilli 
antly  and  be 
comes  infusi 
ble. 

BEFORE    THE    BLOWPIPE.  195 

LIME.     (Continuation  of  page  194.) 


Behavior 

(8) 

1 

Special 

(4) 

(5) 

(6) 

(T) 

reactions. 

in  forceps. 

in  borax. 

in  mic.  salt. 

with  carb.  soda. 

As  on  char 

Gives  the 

As  in  borax. 

Fuses  to  a 

With   micro- 

coal.    Colors 

lime-reaction. 

clear  bead, 

cosmic  salt  in 

the  flame  red. 

opaque  on 

open  tube  gives 

cooling.  With 

the  fluorine- 

an  addition  of 

reaction. 

the  alkali  be 

haves  as  lime. 

196 


BEHAVIOR     OF    MINERAL 

MAGNESIA. 


I 

>  e  h  a  v  i  o  i 

Mineral. 

Formula. 

(1) 

in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

Brucite 

figfi. 

Evolves  water. 

Epsomite 

IVfgS*  -f-  7ft. 

Evolves  water 

Gives  off  HO 

having  an 

and  SO3,  shines 

acid  reaction 

brilliantly,  and 

on  test  paper. 

becomes  alka 

line  and  caus 

tic. 

Boracite  

{lgBa  -f-  2lVIgB 

Occasionally 

Fuses  with 

gives  off  a 

intumescence 

trace  of 

to   a  white 

water. 

crystalline 

bead. 

Magnesite  .  .  . 

«gc. 

Sometimes 
gives   off   a 



Is  infusible. 
With  cobalt- 

small  quantity 

solution,  as 

of  water. 

sumes  a  dusky 

flesh  tint.  ' 

BEFOKE    THE     BLOWPIPE.  197 

MAGNESIA.     (Continuation  of  page  196.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

CO 

with  carb.  soda. 

V. 

Behaves  as 

As  in  borax. 

Behaves  as 

With   nitrate 

magnesia. 

magnesia. 

of  cobalt,  gives 

Sometimes 

the  magnesia- 

gives  a  faint 

reaction. 

iron-reaction. 

V. 

Behaves  as 

As  in  borax. 

The  alkali  is 

The   magne- 

As  on  char 

magnesia. 

absorbed  leav 

siaii  residue 

coal. 

ing  the  mag 

obtained    on 

nesia  on   the 

treating  with 

surface  of  the 

carbonate  of 

charcoal. 

soda  (7),  as 

Gives  the  sul 

sumes  a  flesh- 

phur-reaction 

tint,   when 

on  silver. 

treated  with 

cobalt. 

I. 

Fuses  easily  to 

As  in  borax. 

With  a  small 



As   on   char 

a  clear  bead, 

quantity  of  al 

coal.      Colors 

which  is  crys 

kali  fuses  to 

the  flame 

talline,  when 

a  clear  bead 

green. 

containing 

crystalline  on 

much  of   the 

cooling.  With 

mineral,   and 

a  larger  quan 

is  usually 

tity  gives  a 

slightly  tinted 

clear  uncrys- 

by  iron. 

tallizable 

bead. 

_ 

Behaves  as 

As  in  borax. 

Fuses  to  a 

The    magne- 

magnesia. 

bead,  the  soda 

sian    residue 

Sometimes 

is    then    ab 

obtained   by 

gives  a  slight 
iron-reaction. 

sorbed,  leaving 
an  infusible 

fusing    with 
carbonate   of 

mass  of  mag 

soda  gives  the 

nesia. 

magnesian- 

reaction  with 

nitrate    of 

cobalt.     Dis 

solves    with 

effervescence 

in  warm  HC1, 

198  BEHAVIOR    OF    MINERALS 

MAGNESIA. '  (Continuation  of  page  197.) 


Behavior 

Minpral 

(1) 

(2) 

(3) 

in  glass-bulb. 

in  open  tube. 

on  charcoal. 

Mesitine  spar.  . 

(%Feiln)C. 

As  magnesite. 

___ 

Is  infusible. 

Assumes  a 

• 

deep  brown 

color. 

B  E  F  O  li  E      THE      BLOWPIPE.  199 

MAGNESIA.     (Continuation  of  page  198.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

CO 

with  carb.  soda. 

V. 

Gives  the 
iron  and 
manganese- 
reaction. 

As  in  borax. 

As  magnesite, 
but  the  resi 
dual  mats  has 
a  dark   color 
from  iron  and 
manganese. 

Dissolves  with 
effervescence 
in  warm  HC1. 
With   carbo 
nate  of  soda 
and  nitre  gives 
a  manganese- 
reaction. 

200 


BEHAVIOK,    OF     MINERALS 

ALUMINA. 


Behavior 

Mineral. 

Formula. 

(1) 

(2) 

(») 

in  glass-bulb. 

in  open  tube. 

on  charcoal. 

Sapphire     j 
Corundum  >•  .  . 
Emery        ) 

t 
2L 

— 

— 

— 

Websterite  .  .  . 

*lS  +  9fl. 

Gives  off  water, 

Gives  off  wa 

and,  when 

ter  and  SO3, 

heated  to  inci 
pient  redness, 

leaving  an  in 
fusible  mass. 

sulphurous 

acid. 

Native  Alum.  . 

w+m> 

Intumesces 

Intumesces 

+  24S. 

greatly  and 
gives  off  much 

and   becomes 
infusible. 

water.    Strong 

ly  heated, 

evolves  SO3, 

which  reddens 

litmus. 

Turquoise  .... 

3M+  at 

Evolves  water, 

Turns  brown, 

occasionally 

but  remains    > 

decrepitates 

infusible. 

and  turns 

black. 

BEFORE     THE     BLOWPIPE. 

ALUMINA.     (Continuation  of  page  200.) 


201 


Behavior 

(3) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

co 

with  carb.  soda. 

r 

In   fine   pov,-- 

In  fine  powder 

der  moistened 

dissolves 

with    cobalt- 

V. 

slowly  to  a 

As  in  borax. 



solution  and 

colorless 

heated  as 

glass. 

sumes  a  blue 

- 

color. 

V. 

Behaves  as 

As  in  borax. 

Yields  an  in 

Fused   with 

alumina. 

fusible    mass, 

potassa  in  pla 

which  laid  on 

tinum  has  no 

silver   and 

action  on  sil 

moistened, 

ver.     Cobalt- 

produces  a 

solution    pro 

black  stain. 

duces  the  alu 

mina  reaction. 

V. 

Dissolves  and 

As  in  borax. 

The  alkali  is 

If  not  contain 

Colors  the 

gives  the  iron 

absorbed  into 

ing  much  iron 

flame  violet 

and   manga 

the  charcoal, 

or  manganese, 

if  a  potassa 

nese  reaction, 

leaving  an  in 

gives  an  allu- 

alum  —  yellow 

if  these  oxides 

fusible    mass, 

mina  reaction 

if  soda  —  be 

be   present. 

which    gives 

with    nitrate 

present. 

Otherwise  the 

the    sulphur 

of  cobalt.    In 

bead  is  color 

reaction    on 

other  respects 

less. 

silver. 

as  the  preced 

ing. 

V. 

In  the  oxidiz 

As  in  borax. 

Intumesces, 

Gives  the 

As   on   char 

ing  flame,  gives 

then  fuses  to 

phosphoric- 

coal.     Colors 

a  green  bead, 

a   semi-clear 

acid  reaction. 

the  outer 

due  to  copper 

glass  colored 

flame  green. 

and  iron.     In 

by  iron.  With 

reducing  flame, 

more     alkali, 

opaque  red. 

yields   an  in 

fusible  mass. 

202 


BEHAVIOR     OF     MINERALS 

ALUMINA.     (Continuation  of  page  201.) 


] 

3  e  h  a  v  i  o 

r 

(1) 

(2) 

(3) 

in  glass-bulb. 

in  open  tube. 

on  charcoal. 

Wavellite  .... 

A1F'+3(£1*> 

Evolves  water 

Exfoliates  and 

+182.) 

and  some  fluo 
rine,  which  at 

turns  white. 

tacks  the  glass. 

Spinel  . 

&&1. 

BEFORE    THE     B  L  o  w  p i p  E  . 


203 


ALUMIXA.     (Continuation  of  page  202.) 


Behavior 

(8) 

Qv^^^^l 

(4) 

(5) 

(6) 

cn 

fcpeciai 
reactions. 

in  forceps. 

in  borax. 

in  mic.  salt. 

with  carb.  soda. 

V. 

As   alumina. 

As  in  borax. 

Forms  an  in 

With  cobalt- 

As   on   char 

jenerally  gives 

fusible   white 

solution   on 

coal.     Colors 

also   a   slight 

mass. 

charcoal  gives 

the  outer 

iron  reaction. 

the    alumina 

flame  green, 

reaction. 

especially  if 

moistened 

with  SO3. 

V. 

Gives  a  slight 
iron  reaction. 

As  in  borax. 

Fuses  partially 
and   forms   a 

With  nitrate 
of  cobalt  gives 

porous  mass. 

the    alumina 

reaction. 

With   nitre 

and  carbonate 

of  soda  a  slight 

manganese 

reaction. 

204  BEHAVIOR    OF     MINERALS 

SILICATES. 

The  presence  of  silica  in  a  mineral  can  easily  be  ascertained 
by  treating  a  small  fragment  in  a  bead  of  microcosmic  salt. 
The  bases  will  dissolve  out  with  more  or  less  difficulty  in  the 
salt,  and  the  silica  being  insoluble  will  remain  suspended  in  the 
bead,  retaining  the  original  form  of  the  fragment.  In  borax, 
the  silicates  of  lime  and  magnesia  generally  dissolve  with  con 
siderable  ease,  but  those  of  alumina  slowly  and  with  difficulty. 
The  silicates  of  lime  are  moreover  frequently  characterized  by 
intumescence  or  ebullition,  when  heated  in  the  forceps  in  the 
blowpipe  flame.  The  minerals  presenting  this  character  are 
marked  in  the  table.  As  the  most  convenient  mode  of  classi 
fying  the  silicates  for  blowpipe  examination,  the  following 
arrangement  will  be  adopted  : 

TABLE    I.— ANHYDROUS  SILICATES. 
TABLE  II.— HYDROUS  SILICATES. 

FUSIBILITY. 

I.  Readily  fusible  to  a  bead. 

II.  With  difficulty  fusible  to  a  bead. 

III.  Readily  fusible  on  the  edges. 

IV.  With  difficulty  fusible  on  the  edges. 
V.  Infusible. 

a.  Afford  a  fluid  bead  with  carbonate  of  soda. 

b.  Afford  a  fluid  bead  with  but  little  of  that  salt,  but  with 

a  larger  quantity  a  slaggy  mass. 

c.  Afford  a  slaggy  mass  only. 

This  classification  of  minerals,  according  to  their  fusibility 
and  their  behavior  with  carbonate  of  soda,  was  originally 
proposed  by  Berzelius,  and  a  table  of  the  principal  oxidized 
minerals  arranged  according  to  these  characters  is  given  in  his 
handbook  of  the  blowpipe,  and  thence  adopted,  with  some 
alterations  by  Plattner,  in  the  very  excellent  and  detailed  work 
already  many  times  cited.  In  the  following  general  table  I., 
the  more  important  silicates  only  are  included,  and  in  table  II. 
are  enumerated  in  alphabetical  order  those  which  afford  cha 
racteristic  reactions. 


BEFORE     THE     BLOWPIPE. 


205 


TABLE  I. 

Anhydrous    Silicates. 


Fus.  alon 

and  with 

tfaC. 


I.  a. 


b. 


c. 


II.  a. 


Mineral, 


Axinite , 


Elaolite 

Garnet 

Oligoclase 

Scapolite 

Spodumene 

Asbestos  to  II 

Augite  some  var 

Epidote  to  III 

Hornblende  some  var. 

Sodalite  to  III 

Vesuvian  . , 


Biaxial  Mica  to  III.  .  . 


Hauyne 

Tourmaline  to  V. 


Labrador!  te 

Lepidolite 

Ryacolite , 

Albite 

Augite  some  var. 

Actinolite 

Diopside 

Humboltilite 

Sahlite 

Tremolite 

yrope-. .... 


Formula. 


(SiB) 


NaSi-f^lSi2 
(Ca$a)*§ia-f-23tlSi 

(LiNa)3Si2-f-4£rSi2 
As  Hornblende 
(CaMgFelVrn)3Si2 
(CaFe)3  Si  -f  2(Xl3Pe»n)gi 
(Ca&gFe)4-f  (Si£l)3 
Na3  Si  +  3£lSi  -f  NaCl 


(KNa)3Si  +  3£lSi+tfaSi 


(CaN-aK)Si. 
(KNaL)F-f  (XrFejS'i2  ? 


^3  Si2 

Ca%Fe)4  Si3 
3  Si2 


A.S  Augite 
CaMg)4  Si3 
CaMgFe)3  Si  +  SlSi  -f  mCr? 


206 


BEHAVIOR     OF     M  i  N  E  R  A  L  s 


Fus.  alone 
and  with 

tfaC. 


Mineral. 


Formula. 


III.  a. 


b, 


Anorthite 

Nepheline 

Obsidian 

Orthoclase 

Petalite 

Pumice 

Gadolinite  to  V. 

Nephrite 

Wollastonite  . . 
lolite . . 


IV. 


Beryl 

Diallage 

Hypersthene 
Fuchsite 


V.  a. 
b. 


(Ca&gfraK)3  Si  -f  3(£l£e)Si 


(YCeLaFeCa)3*Si 

Ca3  Si2 


Lcucite 

Chondrodite 

Olivine 

Andalusite 

Chrysoberyl 

Kaynite 

Pycnite | 

Topaz i 

Zircon 

Staurolite  . . 


(Mg,MgF)4  (SiSiF3) 
(MgFeCa)3Si 


Int. 

Int. 
Int. 


BEFORE    THE     BLOWPIPE. 


207 


Hydrous   Silicates. 


Fus.  alone 
and  with 

NaC. 

Mineral. 

Formula. 

I.  a. 

Analcinie.       

fra3Si24-3x.lSi2+6S 

Int. 

Apophyllite  

(K,KF)  (Si,SiF3)4-  6CaSi  -f  15S 

Tnt 

Brewsterite 

(SrBa)Si  +  SlSi3  -f  5& 

Int. 

Chabasite          

(Ca  Na  K)  3  Si9  +  sXlSi"  +  1  8fi 

Int. 

Lapis  Lazuli             .  . 

Si  S  Si  Pe  Ca  Na  £ 

Laumonite  

Ca3  Si2  -f  3SlSi2  -}-  12S 

Int 

Mesotype 

(NaCa)Si  +  SlSi  -f  3^[ 

Int 

Natrolite  

NaSi  -f-  Sl'Si  +  2S 

Int 

Prehnite  
Scolezite  

Ca2Si+Sl§i  +  £[ 
Ca'Si  -f  3tlSi  +  331 

Int. 
Int 

Thomsonite  

(CaNa)3  Si  -f-  33tlSi  +  7S 

Int 

Datholite  

2Ca3  Si  +  B3  Si2  -f  3H 

Int 

Heulandite 

Ca'Si  -f-  SlSi3  -f-  5ll 

Int 

Stilbite 

CaSi  -f  SlSi3  +  6fl 

Int 

b. 

Okenite  

Oa3  Si4  +  6fi 

Int 

Pectolite 

(CJaNa)4Si34-l! 

(3 

Saponite  

2lirg8  Si2  4-  SlSi  +  10  or  6fl 

IT  a 

Antrimolite 

o/p,,-fr\  c:  _i_  KXic;   i   1  Kfr 

b 

Harmatome  
Brevicite 

BaSi4-SlS24-5fl 
"NTaSi  _J_  Xi'q'i  _|_  9T*T 

Orthite  

f?3  Si  j_  ^Si  4-  riT  9^ 

Tnt 

III.  c 

Pitchstone  

5:  XT  3f?p  Tvrp-lSTa  "ft'fl' 

Talc  to  Y 

iCfo-6  >(-;i5  i  o~Fr 

Chlorite  

q  /TVTp-"RW  3  Si  -l-^lIPe^3  Si  4-  Qfi 

Pinite    

^i  Xl  K?P  "RT  TVTo-  "fl" 

208  BEHAVIOR    OF     MINERA 


LS 


Fus.  alone 
and  with 

Sad 

Mineral. 

Formula. 

IV.  a. 

Steatite  

ifrg6  Si5  -f-  4H 

c. 

Gilbertite  

Si  £l  Fe  IVTg  fl 

T_J. 

Meerschaum  

IVIgSi  -f-  E[ 

int. 

Serpentine 

]y[o-fl  Si4  _|-  6"£[ 

V.  a. 

Gismondine  

(CaK)2  Si  -f-  2XlSi  +  9fl 

B 


E  F  O  It  E       THE 


L  O  W  P  I  P  E 


209 


TABLE   II. 


Analeime . . 


Andal 


isite, 


Apophrllite 
Axinite  . . . 


Beryl 

Chabasite... 
Chondrodite 

Chrysoberyl 

Datholite  . . . 
Diallage. . . . 
Fuchsite 

Gadolinite  . . 
Hauyne 

Hypersthene 
Kvanite  .  . 


If  transparent  becomes  white  and  opaque  when  heated,  but 
on  incipient  fusion  resumes  its  transparency  and  then 
fuses  to  a  clear  glass. 

When  powdered  and  treated  with  cobalt  solution  on  char 
coal,  assumes  a  blue  color. 

Fuses  to  a  frothy  white  glass. 

Imparts  a  green  color  to  the  blowpipe  flame,  owing  to  the 
presence  of  boracic  acid.  This  reaction  is  especially  dis 
tinct,  if  the  mineral  be  previously  mixed  with  fluorspar 
and  bisulphate  of 


Sometimes  gives  a  chromium  reaction  in  borax  and  micro- 
cosmic  salt. 

Fuses  to  a  white  enamel. 

Evolves  fluorine  in  the  glass  tube,  both  when  heated  alone 
and  with  microcosmic  salt.  It  sometimes  also  gives  off  a 
trace  of  water. 

Is  unattacked  by  carbonate  of  soda.  With  nitrate  of 
cobalt  on  charcoal  the  finely  powdered  mineral  assumes  a 
blue  color. 

Fises  to  a  clear  glass  and  colors  the  flame  green. 
Frequently  gives  off  water  in  small  quantity. 

Givss  the  chromium  reaction  with  borax  and  microcosmic 

salt. 

That  from  Hitteroe,  if  heated  in  a  partially  covered  plati 
num  spoon  to  low  redness,  glows  suddenly  and  bril 
liantly. 

Affords  the  sulphur  reaction  both  on  charcoal  and  wlu-u 
fused  with  potassa.  It  contains  both  sulphur  and  sul 
phuric  acid. 

As  Diallage. 
As  Andalusite. 


210 


B  E  H  A  V  I  O  It       O  F       M  I  N  K  K  A  L  8 


Lapis  Lazuli 

Laumonite . 
Lepidolite, . 

Leucite  . . . 
Meerschaum 


Okemte.. 
Oli vine  .. 

Pectolite. 
Petalite.. 
Prehnite 
Pycnite. . 

Pyrope . . 

Scolecite. 
Scapolite 

Sodalite . , 


Fuses  to  a  white  glass,  and  when  treated  with  carboiate  of 
soda  on  charcoal,  gives  the  sulphur  reaction  on  silver. 

When  strongly  heated,  exfoliates  and  curls  up. 

Colors  the  blowpipe  flame  crimson,  from  lithia ;  a!so  gives 
the  fluorine  reaction  with  microcosmic  salt. 

Some  varieties,  when  treated  with  cobalt  solution,  assume  a 
blue  color. 

In  the  glass  bulb  frequently  blackens  and  evolves  an  empy- 
reumatic  odor  due  to  organic  matter.  Wh3n  this  is 
burnt  off,  it  again  becomes  white,  and  if  moistened  with 
nitrate  of  cobalt  solution  and  heated,  assurtes  a  pink 
color. 

Behaves  as  Apophyllite. 

Some  varieties  give  off  fluorine,  when  fused  with  micro- 
cosmic  salt. 

Similar  to  Apophyllite. 

Imparts  a  slight  crimson  color  to  the  flame,  like  Lepidolite. 

As  Chabasite. 

Assumes  a  blue  color,  when  treated  with  nitrate  of  cobalt. 
Gives  the  fluorine  reaction  with  microcosmic  salt. 

Gives  the  chromium  reaction  with  borax  and  microcosmic 
salt. 

Similar  to  Laumonite,  but  more  marked. 

Occasionally  contains  a  small  quantity  of  lithia,  and  colors 
the  flame  red  when  fused  with  fluorspar  and  bisulphate 
of  potassa. 

If  mixed  with  one-fifth  its  volume  of  oxide  of  copper, 
moistened  to  make  the  mixture  cohere,  and  a  small  por 
tion  placed  upon  charcoal  and  heated  with  the  blue  oxi 
dizing  flame,  the  outer  flame  will  be  colored  intensely 
blue  from  chloride  of  copper. 


BEFOKE    THE     BLOWPIPE. 


211 


Spodumene 

Stilbite 

Topaz 

Tourmaline 

Wollastonite 
Zircon 


When  not  too  strongly  heated,  colors  the  blowpipe  flame 
red,  when  more  strongly,  yellow. 

As  Chabasite. 

When  heated,  remains  clear.     Otherwise  as  Pycnite. 

Gives  the  boracic  acid  reaction  with  flourspar  and  bisul- 
phate  of  potassa. 

Colors  the  blowpipe  flame  faintly  red  from  lime. 

The  colored  varieties  become  white  or  colorless  and  trans 
parent,  when  heated.  Is  only  slightly  attacked  by  car 
bonate  of  soda. 


212  BEHAVIOR    OF    MINERALS 

URANIUM. 


1 

J  e  h  a  v  i  o  i 

Mineral 

Formula. 

(1) 

(2) 

(3) 

in  glass-bulb. 

in  open  tube. 

on  charcoal. 

Pitchblende... 

TO 

Evolves  some 

Evolves  SO2 

Gives  off  arse 

essentially. 

water  and    a 

and   a  white 

nical  fumes. 

small  quantity 

sublimate  of 

of  sulphur, 

arsenious  acid. 

sulphide  of 

arsenic   and 

metallic 

arsenic. 

Uranium  ochre 

GBP. 

Evolves  water 
and  assumes  a 

— 

V. 

In  reducing 

red  color. 

flame  assumes 

a  green  color. 

(&+£•)£ 

Evolves  water 

_ 

Fuses  with  in 

+  83. 

and  becomes 
yellow  and 

tumescence  to 
a  black  bead 

opaque. 

having  a  semi- 

crystalline 

surface. 

Chalcolite  

(Cu  +  S2)^ 

As  uranite. 

— 

As  uranite. 

+  82. 

BEFORE      THE       BLOWPIPE.  213 

URANIUM.     (Continuation  of  p.  212.) 


Behavior 

(8) 

Special 

(4) 

(6) 

(6) 

(V) 

reactions. 

in  forceps. 

in  borax. 

in  mic.  salt. 

with  carb.  soda. 

III. 

The  roasted 

As  borax. 

Infusible.    Af 

Colors  the 

mineral  affords 

Also  a   small 

fords  the  cha 

flame  blue  be 

the    uranium 

residue  of 

racteristic  Pb 

yond  the  assay, 

reaction. 

silica. 

incrustation, 

owing  to  the 

and  sometimes 

presence  of  Pb. 

yields  minute 

Sometimes  also 

particles  of  Cu. 

green  towards 

the  point,  due 

to  Cu. 



Gives  the 

As  in  borax. 

_ 

. 

uranium 

reaction. 

. 

Gives  the 

As  in  borax. 

Forms  an  in 

Gives  the  PO6 

uranium 

fusible  yellow 

reaction. 

reaction. 

slag. 

As  uranite. 

In  the  oxidiz 

As  in  borax. 

In  reducing 

As  uranite. 

ing  flame  gives 

flame  yields  a 

a  green  bead, 

metallic  bead 

which  in  the 

of  Cu. 

reducing  flame 

becomes  of  an 

opaque   red, 

from  Cu. 

214 


BEHAVIOR    OF    MINERALS 
IRON. 


"IT"                 1 

] 

3  e  h  a  v  i  o 

r 

Mineral. 

Formula. 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

Iron  pyrites.  .  . 

FeS2. 

Gives   a  con 
siderable  yel 

Sulphurous 
acid  and  some 

Gives  off  some 
sulphur,  which 

low  sublimate 

times    arse- 

burns  with  a 

of    sulphur, 

nious   acid 

blue  flame. 

and  sometimes 

are  evolved. 

Residue  fuses 

sulphide  of 

to  a  magnetic 

arsenic.   Also 

bead. 

HS. 

Magnetic  ) 
pyrites    )  "  ' 

fc'fe. 

— 

Evolves  sul 
phurous  acid. 

Fuses  to  a 
magnetic  bead 

black  on  the 

surface,    and 

with  a  yellow 

shining  frac 

ture. 

Mispickel  .  .  •  . 

FeAs-f-FeS2. 

A  red   subli 

Sulphurous  and 

Gives  off  much 

mate  of  AsS2 

arsenious  acids 

arsenic  form 

is  first  formed 

are  evolved, 

ing   a   white 

and    then    a 

the  latter 

incrustation 

black   subli 

forming  a 

and  fuses  to 

mate  of  metal 

white  subli 

a  magnetic 

lic  arsenic. 

mate. 

globule. 

Magnetic  > 

Fea04. 

iron  ore  \  '  '  ' 

Specular  iron.  . 

1     Fea03. 

Red  haematite. 

BEFORE     THE     BLOWPIPE.  215 

IRON".     (Continuation  of  page  214.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6)    - 
in  mic.  salt. 

CO 

with  carb.  soda 

The  roasted 

As  in  borax. 

Fuses  to  a 

mineral  gives 

black  mass, 

a  strong  iron 

which  spreads 

reaction. 

out  on  char 

coal  and  gives 

the  sulphur 

reaction  on 

silver. 

-— 

As  iron  pyrites 

As  in  borax. 

As  iron  pyrites 

— 

— 

As  iron  pyrites 

As  in  borax. 

As  iron  pyrites 

— 

In   the   blue 

Gives  the  iron 

As  in  borax. 

flame,    fuses 

reaction. 

on  edges  and 

remains  mag 

netic. 

1 

V. 

As   magnetic 

As  in  borax. 

— 



;  In    the   blue 

iron  ore. 

flame  is  con 

verted    into 

Fes04,  and 

then  behaves 

as  the   pre 

ceding. 

216  BEHAVIOR     OF     MINERALS 

IROX.     (Continuation  of  page  215.) 


•I 

J  e  h  a  v  i  o  i 

p 

Mineral. 

Formula. 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

Gothite  

Pefi 

Evolves  water 

Frank-Unite  .  .  . 

(FeZnMii) 

Forms  a  white 

(iPe^tn) 

incrustation 

on   the  char 

coal,    which 

moistened 

with    cobalt 

solution   as 

Ilmenite  . 

3ri  and  3?e 

sumes  a  green 
color. 

Chromic  iron  . 
Lievrite  

3(^eCa)3  Si 

Occasionally 

— 

-}-2£eSi. 

gives  off  some 
water  and 

black  globule, 
which  in  the 

turns  black. 

reducing  flame 
becomes 

magnetic. 

Chloropal  .... 

*eSi'  +  8fl. 

Decrepitates 
more  or  less, 

— 

— 

gives  off  much 
water  and 

turns  black. 

B  E  F  O  It  K       T  H  K       B  L  O  W  P  I  P  E  .  2  IT 

IRON.     (Continuation  of  page  216.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

en 

with  carb.  soda. 

As  specular 

As  specular 

As  in  borax. 

iron. 

iron. 

V. 

Gives  the  iron 

As  in  borax. 

Affords  a  con 

Gives  a  strong 

In   the   blue 

and   manga 

siderable  white 

manganese 

flame  fuses 

nese  reaction. 

incrustation  of 

reaction  with 

on  edges 

ZnO. 

nitre  and  car 

and  becomes 

bonate  of  ivoiLi. 

magnetic. 

V. 

Gives  the  iron 

In  oxidizing 

In   reducing 

reaction. 

flame  exhibits 

flame  fuses  on 

the  iron  reac 

edges  and  be 

tion.      In  re 

comes    mag 

ducing   flame 

netic. 

assumes  a  deep 

brownish  red 

color. 

As  the   pre 

Dissolves 

As  in  borax. 

On  platinum 

_ 

ceding. 

slowly    and 

foil  with  nitre 

gives  the 

and  carbonate 

chromium 

of  soda  affords 

reaction. 

a  yellow  mass 

of  chromate 

of  potassa. 

I. 

Gives  the  iron 

Gives  the  iron       Fuses  to  a 

Generally  gives 

In  reducing 
flame  is 

reaction. 

and  silica  re 
actions. 

black  opaque 
bead. 

the  manganese 
reaction  witli 

magnetic. 

nitre  and  c  n1- 

bonatc  of  soda. 

V. 

Gives  the  iron 

Gives  the  iron 

Fuses  to  a 

Loses  color 

reaction. 

and  silica  re 

transparent 

and    turns 

actions. 

green  glns.s. 

black. 

218  B  E  II  A  V  i  O  II       O  F       M  I  JS'  E  K  A  L  S 

IKON.     (Continuation  of  page  217.) 


Jb  ormulti. 

I 

J  e  h  a  v  i  o  i 

Mineral. 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 

on  charcoal. 

Green  earth  .  . 

Si,Fe,£l,Na, 

jives  off  water 

. 

_ 

±,fl,  etc. 

and   becomes 

darker  in 

color. 

Siderite 

FeC. 

Occasionally 

As   in   glass 

decrepitates. 

bulb. 

Gives  off  CO2 

and  turns 

black  and 

magnetic. 

Copperas  

FeS-f7fi. 

Gives  off  wa 
ter,  and,  when 

Evolves  water 
and   S0a, 

Loses  water 
and  SO3,  and 

strongly  heat 

which  may  be 

is  converted 

ed,   SO'2  and 

recognized  by 

into  F"e. 

SO3,  which 

its  odor. 

redden  litmus 

paper. 

Vivianite  

Fe'lP  +  811. 

Gives   off 
water. 

Froth?  up  and 
then  fuses  to 

a  grey  metal 

lic  bead. 

1 

BEFOKE     THE     BLOWPIPE  219 

IROX.     (Continuation  of  page  218.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

cn 

with  carb.  soda 

V. 

As  the  pre 

As   the   pre 

Forms   a 

In    reducing 
flame  fuses  on 

ceding. 

ceding. 

slaggy  mass. 

edges  and  co 

lors  the  outer 

flame   yellow 

(N&)  or  violet 

(K). 

Behaves  simi 

Gives  the  iron 

As  in  borax. 

Behaves  as  an 

In  acid  dis 

larly  to  the 

and  sometimes 

oxide.     With 

solves   with 

magnetic 

manganese 

nitre  and  car 

effervescence. 

oxide. 

reaction. 

bonate  of  soda 

on  platinum 

generally  gives 

the  manganese 

reaction. 

Gives  off  H 

The  roasted 

As  in  borax. 

Forms   sul 

If  dissolved  in 

and  SO2,  and 
then  behaves 
as  the  magne 

mineral  affords 
an  iron  reac 
tion. 

phide  of  so 
dium  and 
oxide  of  iron. 

water,  and  a 
strip  of  silver- 
foil  be  intro 

tic  oxide. 

The  former  is 

duced  into  the 

absorbed  into 

solution,    the 

the  charcoal, 

metal  remains 

and  if  cut  out 

untarnished. 

and  laid  upon 

silver  and 

moistened 

gives  the 

S  reaction. 

As  on  char 
coal.     Singes 

Gives  the  iron 
reaction. 

As  in  borax. 

In  reducing 
lame  becomes 

— 

flame  green 

magnetic  and 

(£)- 

fuses  to  a 

black  slaggy 

mass. 

220 


BEHAVIOR     OF     MINERALS 
IRON.     (Continuation  of  page  219.) 


Mi  n  Ami 

] 

3  e  h  a  v  i  o 

r 

JZuUt/Falc 

(1) 

in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

Iriphyline  

(FeMnLi)3£. 

Gives  off  wa 

_ 

Fuses  readily 

ter,  having  an 

to    a   black 

alkaline  reac 

magnetic  bead 

tion,  and   as 

with  a  metal 

sumes   a  me 

lic  lustre. 

tallic   lustre 

resembling 
graphite. 

Scorodite  . 

3Pels-f  4fl. 

Evolves  water. 

Gives  off  water 

Emits  arseni 

and  AsO3. 

cal  fume  and 

in  the  reduc 

ing   flame 

fuses  to  a 

magnetic  mass 

having  a  me 

tallic  lustre. 

Cube  ore  

Fe8ls+3Pe3ls2 

Evolves  much 

As  the   pre 

As   the  pre 

+  18fl. 

water. 

ceding. 

ceding. 

B  E  F  O  II  E       T  HE       B  L  O  W  P  I  P  E  . 


IRON.     (Continuation  of  page  220.) 


Behavior 

(8) 

Q^rt^r.1 

(4) 

(5) 

(6) 

W 

bpecial 
reactions. 

in  forceps. 

in  borax. 

in  mic.  salt. 

with  carb.  soda. 

I. 

Gives  the  iron 

Gives  the  iron 

Forms  an  in 

Gives  the 

On  platinum 

and  manganese 

reaction  which 

fusible  porous 

manganese 

wire  colors  the 

reactions. 

overpowers 

mass,  which 

reaction  with 

flame  crimson 

that  of  the 

under  the  re 

nitre  and  car 

(Li)  and  green 

manganese. 

ducing  flame 

bonate  of  soda 

(1^),    towards 

becomes  mag 

on   platinum 

the  point  fuses 

netic. 

foil. 

to    a   black 

magnetic 

bead. 

s 

I. 

The  roasted 

As  in  borax. 

As   alone   on 

Gives  the  arse 

As  on  char 

mineral  gives 

charcoal. 

nic  reactions. 

coal.     Colors 

an  iron  reac 

the  outer  flame 

tion. 

blue. 

!  As  the   pre 

As  the  pre 

As  in  borax. 

As  the  pre 

As  the  pre 

ceding. 

ceding. 

ceding. 

ceding. 

i 

222  BEHAVIOE     OF    MINERALS 

MANGANESE. 


Mineral. 

Formula. 

J 

3  e  h  a  v  i  o 

p 

(1) 

(2) 

(3) 

in  glass-bulb. 

in  open  tube. 

on  charcoal. 

Manganblende 

MnS. 

— 

Gives  off  SO2 
and  becomes 

[s  slowly  roast 
ed  and  con 

greyish  green 

verted  into 

on  surface. 

oxide. 

Pyrolusite  .... 

fin. 

Frequently 

gives   off  a 

small  quantity 

of  water  and, 

when  strongly 
lieated,  oxygen. 

Manganite.  .  .  . 

MnH. 

Gives  off  much 

— 

— 

water. 

Psilomelane  .  .  . 

(Ba,Ca,fig,K) 

Gives  off  water 

.  —  . 

__ 

fin  -f-  S. 

and,   when 

strongly  heat 

ed,  oxygen. 

Wad  

fin,Mn,fl, 

Gives  off 

also 

water. 

Pb,Si,  etc. 

I 

BEFORE    T  11  E     B  L  o  w  r  i  p  E  . 


223 


MANGANESE.     (Continuation  of  page  222.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

0) 

with  carb.  soda. 

V. 

The   roasted 

In  the  un- 

Forms  a  slaggy 

_ 

mineral  gives 

roasted  state, 

mass,  which 

a  strong  man 

dissolves  with 

laid  on  silver 

ganese  reac 

much    ebulli 

and  moistened, 

tion. 

tion   and   de 

gives  the  sul 

tonation  due 

phur  reaction. 

to   the  elimi 

nation  of  sul 

phide  of  phos 

phorus.     The 

bead  then  ex 

hibits    the 

characteristic 

violet  color  of 

manganese. 

V. 

Gives  the 

As  in  borax. 

Forms  a 

. 

manganese 

slaggy  mass. 

reaction. 

V. 

Exfoliates 

As  the   pre 

As  in  borax. 

As  the  pre 

— 

slightly. 

ceding. 

ceding. 

Y. 

As  pyrolusite. 

As  in  borax. 

As  pyrolusite. 



Colors   flame 

faintly  green 

(Ba)  and  red 

towards^  the 

point  (Ca). 

V. 

Colors  flame 

Gives  the 
manganese 

As  in  borax. 

As  pyrolusite. 

Various  ac 
cording   to 

variously  ac 

reaction,  more 

composition. 

cording  to  its 

or  less  modi 

When  strongly 

composition. 

fied  by  the 

heated    and 

presence   of 

;hen  moistened 

other  oxides. 

las  an  alkaline 

reaction  on  red 

litmus  paper. 

224:  BEHAVIOR     OF     MINERALS 

MANGANESE.     (Continuation  of  page  223.) 


Behavior 

Mineral. 

Formula. 

(1) 

(2) 

(°) 

in  glass-bulb. 

in  open  tube. 

on  charcoal. 

Rhodonite.  .  .  . 

&n3Si2. 

Gives  off  more 

_ 

Under  a  strong 

or  less  water. 

flame  fuses  to  a 

brown  opaque 

bead. 

Diallogite  .... 

MnO. 

Frequently 
decrepitates 
and  gives  off 

— 

If  strongly 
heated   and 
moistened  has 

more  or  less 

an   alkaline 

water. 

reaction   on 

litmus   paper 

due   to   the 

presence  of  Ca. 

Triplite  

(MnFe)4£. 

1  Generally  gives 

— 

— 

off  more   or 

less  water. 

BEFORE     THE     BLOWPIPE.  225 

MANGANESE.     (Continuation  of  page  224.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

CO 

with  carb.  soda. 

II. 

In  the  oxidiz 

As  in  borax, 

With  a  small 

As   on  char 

ing  flame  gives 

but  leaves  an 

quantity  of  the 

coal. 

the  manganese 

insoluble  sili 

alkali  fuses  to 

reaction.     In 

ceous  skeleton. 

a  black  bead. 

reducing  flame 

With  a  larger 

the  iron  reac 

quantity  forms 

tion  more  or 

a  slag. 

less  intense. 

Y. 

Gives  the 

As  in  borax. 

Forms  an  in 

In  warm  acid 

Frequently 

manganese 

fusible  slag. 

dissolves  with 

colors  the 

and  iron  reac 

much   effer 

flame  slightly 

tions. 

vescence. 

red. 

I. 

Colors    the 

Gives  the 

As  in  borax. 

Forms  an  in 

— 

outer  blowpipe 

manganese 

fusible  mass. 

flame   green 

and  iron  reac 

c?>. 

tions. 

10* 


226 


BEHAVIOR     OF     MINERALS 
NICKEL    AND     COBALT. 


Mineral. 

Formula. 

] 

3  e  h  a  v  i  o 

r 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

Millerite  

NiS. 

Evolves  SO2. 

Fuses  with 

much  ebulli 

tion  to  a  mag 

netic  bead. 

Coppernickel... 

Ni2As. 

Gives  off  a 

Gives  off  much 

Fuses  to  a 

little  AsO3. 

AsO3  and 

magnetic  bead, 

some  SO2  and 

with  the  evo 

falls  to  powder. 

lution  of  arse 

nic,  which 

colors  the 

flame  blue. 

Smaltine  

CoAs. 

When  strongly 

Gives  a  crys 

Gives  off  fumes 

heated   gene 

talline  subli 

of  arsenic,  and 

rally  evolves 

mate  of  AsO3. 

fuses  to  a  dark 

metallic 

Also  some  SO2. 

grey  magnetic 

arsenic. 

bead,  very 

brittle,  colors 

flame  blue. 

BEFORE    THE     BLOWPIPE. 

NICKEL   AND   COBALT.     (Continuation  of  page  226.) 


227 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(«) 

in  mic.  salt. 

p) 

with  carb.  soda 

The  roasted 

As  in  borax. 

Fuses  to  a 

mineral  gives 
a  nickel  reac 

slaggy  mass, 
which  on  sil 

tion,   slightly 
modified  by 

ver  gives  the 
sulphur  reac 

small  quanti 

tion. 

ties  of  iroii 

and  copper. 

_ 

The  arsenical 

If  the  residual 

___ 

Affords  a  sub 

bead  obtained 

bead  which 

limate  of  me 

by  fusing  the 

has   been 

tallic    arsenic 

mineral   on 

treated   with 

when  treated 

charcoal,  if 

borax  be  fur 

with   cyanide 

fused   upon 
the  same  sup 

ther  treated 
with  microcos- 

of  potassium. 

port   with 

mic   salt,  the 

borax  succes 

nickel  reaction 

sively  added 

will  be  obtain 

and  removed, 

ed  and  some 

gives  firstly  an 

times  a  slight 

iron  reaction, 

copper    reac 

then  cobalt  if 

tion. 

present,  and 

lastly  nickel. 

_ 

As   the  pre 

Gives  the  co 

As  the   pre 

ceding,  but  the 
cobalt  being  in 

balt  reaction, 
and  after  the 

ceding. 

large  excess 

cobalt    has 

requires  some 

Deen  removed, 

time   for   its 

that  of  nickel. 

perfect  oxida 

tion,   before 

~ 

the  nickel  re 

action  is  ex 

hibited. 

B  K  ii 


A  V  I  O  K       O  F 


MINERALS 


NICKEL   AND   COBALT.     (Continuation  of  page  22*7.) 


Mineral. 

Formula. 

Behavior 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

Glance  cobalt 

CoS2  +  CoAs. 

As   the  pre 

Gives   off  S 

ceding,    but 

and  As,  and 

gives  off  more 

fuses   to   a 

SO2. 

magnetic 

bead.    Colors 

flame  blue. 

Nickel  glance 

NiS2  -f  NiAs. 

Decrepitates 
and  gives  an 

As   the   pre 
ceding. 

As  the  pre 
ceding. 

orange  color 

ed    sublimate 

of  AsS3. 

Ulmannite.  .  .  . 

NiS2  +  Ni 
(AsSb)2. 

Gives  a  slight 
white   subli 
mate  of  SbO3 

Gives  off  thick 
fumes  of  SbO3 
and  SbO5  with 

As  glance  co 
balt,  but  ac 
companied  by 

and   more  or 

AsO3  and  SO2. 

dense   fumes 

less  AsS3. 

of  SbO3. 

Cobalt  pyrites 

(CoNiFe) 
(<3o'$iFe)- 

When  strongly 
heated  gives 
off  sulphur 
and  becomes 

Gives  off  much 
SO2  and  a 
small  quantitv 
of  AsO3. 

In  the  reduc 
ing  flame  small 
fragments  fuse 
with  the  evo 

brown. 

lution  of  sul 

phur  to  a  mag 

netic  bead 

having  a 

bronze  colored 

fracture. 

Emerald  nickel 

fti3<j  _|_  cfl.     Gives  off  much 

— 

— 

water  and 

turns  black. 

BEFORE     T  H  i;     1>  L  o  w  P  i  v  K  . 
NICKEL    AXD   COBALT.     (Continuation  of  p.  228.) 


229 


Behavior 

(3) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

(V) 
vith  carb.  soda. 

Gives  a  cobalt 

As  in  borax. 

Gives   a   sul 

As  the   pre 

and  slight  iron 

phur  reaction 

ceding. 

reaction  when 

of  silver. 

treated  as  the 

preceding 

minerals. 

_ 

As  copper 

Gives  the 

As  the   pre 

As  copper 

nickel. 

nickel  reaction, 

ceding. 

nickel. 

occasionally 

somewhat 

obscured  by 

, 

cobalt. 

As  copper 

As  the   pre 

As   the  pre 

As  copper  nic 

nickel. 

ceding. 

ceding. 

kel  generally, 

but  arsenic  is 

not  always 

present. 

_ 

In  the  oxidiz 

As  in  borax, 

As  glance 

As  copper 

ing  flame   on 

but  the  reduc 

cobalt. 

nickel,  but  the 

charcoal  gives 

tion    of    the 

amount  of  ar 

a  violet  colored 

nickel  is  more 

senic  is  usual 

glass.      In   the 

difficult   than 

ly  very  small. 

reducing  flame 

in   the   latter 

the  nickel  is  re 

flux. 

duced  and  may 

be  collected  in 

a  gold  bead. 

When  the  nic 

kel  is  removed, 

the  glass  exhi 

bits   a   slight 

iron  reaction 

while  warm. 

Dissolves  with 

As  in  borax. 

Forms   a 

In  warm  dilute 

much  efferves 

slaggy  mass. 

HC1  dissolves 

cence  and  gives 
the  nickel  re 

with   much 
effervescence. 

action. 

230  BEHAVIOR     OF     MINERALS 

NICKEL  AND   COBALT.     (Continuation  of  page  229.) 


Behavior 

Mineral. 

Formula. 

(1) 

(2) 

(3) 

in  glass-bulb. 

in  open  tube. 

on  charcoal. 

Cobalt  bloom.  . 

Co3ls  -f-  83. 

Gives  off 



Evolves  arse 

water 

nical   fumes 

and   in   the 

reducing  flame 
fuses  to  a  dark  1 

grey  bead  of 

arsenide    of 

cobalt. 

Earthy  cobalt.  . 

$Tn,Oo,<X 
Fe,S,  etc. 

Gives  off 
water. 

— 

Emits  a  slight 
smell  of  arse 
nic,  but  does 

not  fuse. 

BEFORE     THE     BLOWPIPE. 

NICKEL  AND   COBALT.     (Continuation  of  page  230.) 


231 


Behavior 

(8) 

(4) 

(5) 

(6) 

CO 

Special 
reactions. 

in  forceps. 

in  borax. 

in  mic.  salt. 

with  carb.  soda. 

In  the  point 

Gives  the  co 

As  in  borax. 

_ 

Gives   off* 

of  the   blue 

balt  reaction. 

arsenic  with 

flame  fuses 

cyanide    of 

and  colors  the 

potassium  in 

outer  flame 

glass  tube. 

blue  (As). 

Colors  the 

In  oxidizing 

As  in  borax. 

Forms  an  in 

With   carbo 

flame  blue. 

flame   gives 

If  a  saturated 

fusible   mass. 

nate  of  soda 

the  cobalt  re 

bead  be  treat 

and   nitre   on 

action    which 

ed    on   char 

platinum  foil, 

obscures  those 
of  Mn,Cu,  etc. 

coal  with  tin 
in  the  reduc 

gives  a  strong 
manganese 

In   reducing 

ing  flame  for 

reaction. 

flame  occa 

a  few^seconds, 

sionally  gives 

the  Cu  reac 

the  Cu  reac 

tion  is  some 

tion. 

times  obtained. 

232  BEHAVIOR     OF     MINERALS 

ZINC. 


Mineral. 

I 

J  e  h  a  v  i  o  i 

Formula. 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

Zincblende  .  .  . 

ZnS. 

Decrepitates 

Evolves   SO 

V. 

strongly. 

and  becomes 

In  the  reduc 

white  or  yel 

ing  flame 

low  if  contain 

incrusts   the 

ing  iron. 

charcoal  with 

ZnO;  also 

with  CdO,  if 

that  metal  be 

present. 

Red   oxide  of 

2n. 

In  the  reduc 

ing  flame 

forms   a  thin 

incrustation 

of  oxide  of 

zinc  on   the 

charcoal. 

Electric    calu- 

22n3Si-f3ll. 

Gives  off  water 

_ 

miue  

and   becomes 

white  and 

opaque. 

Calamine  

2nC. 

Gives  off  CO2 

As  the  red 

and  becomes 

oxide.   Some 

opaque. 

times  also 

gives  a  cad 

mium  and 

•*  . 

lead  incrusta 

tion. 

B  E  F  O  E  E       THE       B  L  O  W  T  I  P  E  .  233 

ZIXC.     (Continuation  of  page  232.) 


Behavior 

(8) 
Special 
reactions. 

(-1) 
in  forceps 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

m 

with  carb.  soda. 

_ 

The  roasted 

As  in  borax. 

As   alone   on 

mineral  gives 

charcoal. 

a  zinc  reaction, 

Moreover  co 

ind  sometimes 

lors  the  flame 

a  slight  iron- 

blue.     The 

reaction. 

fused    alkali 

gives  a  S  reac 

tion  on  silver. 

V. 

Generally  gives 
a  manganese 

As  in  borax. 

On    charcoal, 
forms  a  thick 

With  carbo 
nate  of  soda 

and  slight 

incrustation 

and  nitre  on 

iron  reaction 

of  ZnO. 

platinum  foil 

in  addition  to 

gives  a  man 

that  of  zinc. 

ganese  reac 

tion. 

V. 

Dissolves   to 

Dissolves  to  a 

With  carbo 

a  clear  glass, 

clear   glass, 

nate  of  soda 

which  cannot 

which  becomes 

alone  is  infu- 

be  rendered         opaque  on       sible.   With  2 

opaque  by  the 

cooling.     Silica:  parts  of  alkali 

intermittent 

remains   in-     and  1  of  borax 

flame. 

soluble. 

fuses  to  a  glass 

and  sets  free 

2n,  which 

incrusts  the 

charcoal. 

V. 

Gives  a  zinc 

As  in  borax. 

Forms  a  thick 

Dissolves  with 

reaction  and 

incrustation 

much  efferves 

frequently  an 

of  zinc,  some 

cence  in  cold 

iron  and  man 

times  also  of 

acid. 

ganese  reac 

fb  and  Co. 

tion. 

i 

234:  BEHAVIOR     OF     MINERALS 

BISMUTH. 


Mineral. 

Formula. 

Behavior 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

Native  bismuth 

Bi. 

— 

Fuses  and   is 

Fuses  to  a 

converted  into 

bead  and  in- 

a  yellow  oxide. 

crusts   the 

charcoal  with 

oxide. 

Bismuthine  .  .  . 

BiS. 

— 

Fuses  with 

Fuses  with 

ebullition  and 

much  spirting 

gives  off  S  and 

and  in  the  re 

SO2. 

ducing   flame 

yields  a  me 

tallic  bead  and 

incrusts   the 

charcoal,  with 

oxide. 

Bismuthblende 

Bi'Si3. 

Turns  yellow 

__ 

Fuses  \\ith 

and,  when 

ebullition  to  a 

strongly  heat 

brown   globule 

ed,  fuses. 

forming   an 

incrustation 

of  Si  on  the 

charcoal. 

BEFORE     THE     BLOWPIPE.  235 

BISMUTH.     (Continuation  of  page  234.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

m 

with  carb.  soda. 

__ 

The  oxide 

As  in  borax. 



_ 

formed   upon 

charcoal  gives 

the   bismuth 

reactions. 

— 

The  oxide  ob 

As  in  borax. 

As  alone   on 



tained  upon 

charcoal  The 

charcoal  gives 

fused  alkali 

the  bismuth 

gives  the  sul 

reactions. 

phur  reaction 

on  silver. 

I. 

Gives  the  bis 

As  in  borax, 

Fuses  to  a 

Fuses  with 

muth  and  also 

but  leaves  a 

yellow  mass. 

ease  to  a  yel 

an  iron  reac 

silicious    ske 

The   bismuth 

low  bead,  co 

tion. 

leton. 

is  then  reduced 

loring  the 

to  the  metal 

outer  flame 

lic  state  and 

bluish  green, 

partially  vola 

especially   if 

tilized,  incrust- 

moistened 

ing  the  char 

with  HC1. 

coal  beyond. 

This  color  is 

due  to  £. 

236 


BEHAVIOR     OF     MINERALS 


BISMUTH.     (Continuation  of  page  235.) 


Behavior 

Mineral. 

Form  u.1  ci 

(1) 

(2) 

(3) 

in  glass-bulb. 

in  open  tube. 

on  charcoal. 

Tetradymite  .  . 

Bi,Te,S. 

Occasionally 

Fuses  and 

Fuses  to  a 

decrepitates 

gives  off'  white 

metallic  bead, 

and  then  fuses, 

fumes,  part  of 

colors  the 

forming   a 

which  pass  up 

outer   flame 

greyish  white 

the  tube  and 

bluish  green 

sublimate  im 

part   deposit 

(Te   and   Se) 

mediately 

immediately 

and  incrusts 

above   the 

above  the 

the  charcoal 

mineral  frag 

mineral.    This 

around   with 

ment. 

latter  if  heated,  the  orange  -Bi, 

fuses  to  clear 

beyond  which 

drops  (TeO3). 

is  a  white  in 

The  mineral  re 

crustation  part 

sidue  becomes 

ly  consisting 

surrounded  by 

of  Te. 

fused  Si,  cha 

racterized  by 

its   yellow 

color. 

B  E  F  O  K  E      THE       BLOWPIPE.  237 

BISMUTH.     (Continuation  of  page  236.) 


Behavior 

(8) 
Special 

(4) 

(5) 

(6) 

en 

reactions. 

in  forceps. 

in  borax. 

in  mic.  salt. 

with  carb.  soda. 

The  yellow 
oxide  obtained 
upon  charcoal 
gives  the  bis- 
nuth  reaction, 
and  the  white 
incrustation 
that   of  bis 
muth  and  tel 
luric  acid. 

As  in  borax. 

[n  the  reducing 
flame  yields  a 
bead   of  me 
tallic  bismuth, 
part  of  which 
is  with  part  of 
the  tellurium 
volatilized  and 
incrusts  the 
charcoal 

The  fused  alka- 
ine  mass  gives 
the    sulphur 
reaction   on 
silver.     Also 
gives  the  tellu 
rium  reaction 
with  charcoal 
and  carbonate 
of  soda. 

around. 

238 


BEHAVIOK     OF     MINERALS 
LEAD. 


Mineral. 

Formula. 

Behavior 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 

on  charcoal. 

Galena  

PbS. 

Generally  de 

Gives  off  SO2, 

Fuses  and   is 

crepitates  and 

and    when 

reduced  afford 

gives   off  a 

strongly  heat 

ing  a  bead  of 

small  quantity 

ed,   a   white 

metallic  lead, 

of  sulphur. 

sublimate    of 

and  forming 

Pb,S. 

an  incrustation 

of  PbO  on  the 

charcoal.    Co 

lors  the  outer 

flame  blue. 

Clausthalite  .  .  . 

PbSe. 

Decrepitates 

Forms  a  sub 

Gives  off  fumes 

slightly. 

limate  of  se 

smelling 

lenium,  which 

strongly  of 

is  grey  when 

selenium  and 

thickly  depo 

coloring   the 

sited,  and  red 

flame  blue. 

when  thin. 

In  the  reduc 

ing  flame  fuses 

partially  and 

incrusts  the 

charcoal  with 

Se   and  PbO. 

After   some 

time  a  black 

infusible  mass 

alone  remains. 

Jaracsouite  .  .  . 

Pb'Sb*. 

Fuses  and  gives 

Fuses  and 

Fuses  with 

off  some  sul 

emits  dense 

great  ease 

phur,  sulphide 

white  fumes  of 

evolving  much 

of  antimony      SbO3,   which 

SbO3  and  PbO, 

and  antimony     pjuss    off  and 

which  incrusts 

which    con-        redden  blue 

the   charcoal 

dense  in  the      litmus  Daoer. 

around    the 

neck  of  the 

mineral.  When 

bulb. 

the  fumes  have 

ceased,  a  small 

bead   of  me 

tallic   lead 

remains. 

B  E  F  O  JB  E       THE       BLOWPIPE. 
LEAD.     (Continuation  of  page  238.) 


239 


Behavior 

(8) 

Special 

(4) 

(5) 

(6) 

cn 

reactions. 

in  forceps. 

in  borax. 

in  mic.  salt. 

with  carb.  soda. 

The  oxide 

As  in  borax. 

As   alone    on 



formed    upon 
charcoal  gives 
the  lead  reac 

charcoal.  The 
fused  alkali 
gives  a  sul 

tion. 

phur  reaction 

on  silver. 

The  infusible 

As  in  borax. 

With  carbonate 

residue  obtain 

of  soda,  or  ox- 

ed  upon  char 
coal  gives  an 
iron  and  some 

alate  of  potash 
yields  a  metal 
lic  bead,  the 

times   copper 
and  cobalt  re 

fused  alkali 
laid  upon  sil 

action. 

ver  and  mois 

tened  produces 

a  stain  similar 

to   that   pro 

duced  by  sul 

phur. 

— 

The   yellow 
incrustation 
formed  upon 
charcoal  gives 
the  reaction  of 

As  in  borax. 

As   alone    on 
charcoal.  The 
fused   alkali 
gives  the  sul 
phur  reaction 

— 

lead,  and  the 

on  silver. 

^ 

white  those  of 

antimony. 

i 

BEHAVIOK     OF     MINERALS 

LEAD.     (Continuation  of  page  239.) 


Mineral. 

Formula. 

Behavior 

CD 

in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

Minium 

Pb304. 



_ 

Is  reduced  first 

to  litharge 

(PbO)  and  then 

to  metallic  leac 

which  forms 

the  usual  in 

crustation. 

Mendipitc  .... 

]  PbCl  -f-  2PbO. 

Decrepitates 
sliglitly  and 

— 

Fuses  readily 
jand  is  reduced 

i 

assumes  a 

to  metallic 

yellow  color. 

lead  with  the 

evolution  of 

acid  fumes. 

Forms  a  white 

incrustation 

of  PbCl,  and 

a  yellow  one 

of  PbO. 

pb<3. 

Decrepitates, 

— 

Is  reduced  to 

gives  off  CO2, 

metallic  lead, 

turns  yellow, 

incrusting  .the 

and  fuses. 

charcoal 

around  with 

PbO. 

Anglesite  

PbS. 

Decrepitates 

— 

In  the  oxidiz- 

and  gives  off 

ng  flame  fuses 

a  small  quan 

to  a  clear  bead, 

tity  of  water. 

which  becomes 

opaque  on 

cooling.     In    ! 

reducing  flame 

is  reduced 

with  much 

ebullition  to 

i  metallic  bead 

and  incrusts 

the  charcoal 

around    with 

PbO. 

B  E  F  O  K  E       THE       BLOWPIPE. 
LEAD.     (Continuation  of  page  240.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

CO    " 
with  carb.  soda. 

Colors  the 

Gives  the  lead 

As  in  borax. 

As   alone   on 

outer   flame 

reactions. 

charcoal. 

blue. 

As  the  pre 
ceding. 

As   the  pre 
ceding. 

As  ia  borax. 

As   alone    on 
charcoal. 

Gives  the  chlo 
rine    reaction 

with  CuO  and 

. 

microcosmic 

, 

salt. 

As  the   pre 

Gives  the  lead 

As  in  borax. 

As  alone    on 

^ 
In  nitric  acid 

ceding. 

reaction. 

charcoal. 

dissolves  with 

much  effer 

vescence. 

As  the   pre 

Gives  the  lead 

As  in  borax. 

Is  reduced 

ceding. 

reaction  and 

yielding  a 

occasionally  a 

metallic  lead 

slight  iron  and 

bead.      The 

manganese 

fused  alkaline 

reaction. 

mass  gives  a 

sulphur  reac 

tion  on  silver. 

!i 


24:2 


BEHAVIOR     OF    MINERALS 


LEAD.     (Continuation  of  page  241.) 


Mineral. 

Formula. 

E 

(1) 
in  glass-bulb. 

e  h  a  v  i  o  r 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

Pyromorphite 

PbCl-f  3Pb3P\ 

Decrepitates, 
and  when 
strongly  heat 
ed   for   some 
time,  gives  a 
slight  white 
sublimate  of 
PbCl. 

In  oxidizing 
flame  fuses  to 
a  bead  having 
a  crystalline 
surface  on 
cooling,  and 
forms  a  thin 
film   of  PbCl 
on  the  char 

coal.      In  re 

ducing   flame 
fuses  without 

reduction  and 

«• 

on  cooling  as 
sumes  a  poly 
hedral  form. 

Incrusts  the 

.  T 

charcoal 

slightly  with 
PbO. 

Mimetene  .... 

PbCl-f3Pb3ls 

As  the  pre 
ceding. 

Fuses,  but  less 
easily  than  the 
preceding, 
gives  off  AsO3 
and  incrusts 

the  charcoal 

with  PbCl. 

Finally  is  re 
duced   to    a 

metallic  bead 

and  forms  an 

incrustation 
of  PbO. 

BEFORE    THE     BLOWPIPE.  243 

LEAD.     (Continuation  of  page  242.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

(?) 

with  carb.  soda. 

Fuses  and  co 

. 

__ 

Is  reduced 

Gives  the  chlo 

lors  the  flame 

yielding  a 

rine   reaction 

blue. 

metallic  bead 

with  microcos- 

and  incrusting 

mic   salt   and 

the  charcoal 

CuO.  Also  the 

with  PbO. 

phosphoric 

acid  reactions. 

As  the  pre 

The  oxide 

•* 
As  iii  borax. 

As  the  pre 

Gives  the  chlo 

ceding. 

formed  on 

ceding. 

rine  reaction. 

charcoal  gives 

the  lead  reac 

tions. 

24:4:  BEHAVIOR    OF    MINERALS 

LEAD.     (Continuation  of  page  243  ) 


j 

I 

J  e  h  a  v  i  o  i 

Mineral. 

Formula. 

(i) 

(2) 

(3) 

in  glass-bulb. 

in  open  tube. 

on  charcoal. 

Vanadinite  .  .  . 

PbCl-f3Pb3V  ? 

As  pyromor- 
phite. 

— 

The  powdered 
mineral  fuses 

to  a  black 

shining  mass, 

which  in  the 

educing  flame 

affords  a  me 

tallic  bead. 

Incrusts  the 

charcoal  first 

with  a  white 

film  of  PbCl 

and  afterwards 

with  PbO. 

Crocoisite  

*bOr. 

Decrepitates 
violently  and 

— 

Fuses  and  de 
tonates,  yield 

issuuies  a  dark 

ing  C203  and 

color. 

metallic  lead, 

and  forming 

an  incrustation 

of  PbO  on  the 

charcoal. 

Molybdate   of 

pbM. 

As  the  pre 
ceding. 

- 

Fuses  and  is 
partly  absorb 

ed  into  the 

charcoal  leav 

ing  a  globule 

of  metallic 

lead,  which  is 

partially  oxi 

dized  and  in- 

crusts  the 

charcoal. 

BEFORE     THE     BLOWPIPE.  215 

LEAD.     (Continuation  of  page  244.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

(?) 

with  carb.  soda. 

As  pyromor- 
phite. 

Dissolves  rea 
dily  to  a  clear 
glass,    which, 

In  oxidizing 
flame  is  yellow 
while  hot,  be 

On    platinum 
wire  fuses  to 
a  yellow  bead, 

With  micro- 
cosmic  salt  and 
CuO,  gives  the 

in  the  oxidiz 

coming  paler 

which  is  crys 

chlorine  reac 

ing   flame,   is 

on   cooling. 

talline   on 

tion.    If  fused 

yellow   while 

In  reducing 

cooling.     On 

in  a  platinum 

hot,  and  color- 

flame  brown 

charcoal  yields 

spoon  with 

ess  when  cold. 

while  warm, 

a  button  of 

from   3   to  4 

In    reducing 

and  emerald 

metallic  lead. 

times  its  vo 

flame  becomes 

green  when 

lume  of  K,S2 

opaque,  and  on 

cold. 

it  forms  a 

cooling  green. 

fluid  yellow 

mass  having 

an  orange  co 

lor  when  cold. 

As  pyromor- 

Dissolves  rea 

As  in  borax. 

On  platinum 

Treated  as 

phite. 

dily  and  colors 

foil   gives   a 

above   with 

the  glass  yel 

dark  yellow 

K,S2  forms  a 

low  while 

mass,  which 

violet  colored 

warm,   and 

becomes  paler 

mass,  which 

green  when 
cold. 

on    cooling. 
On   charcoal 

on  solidifying 
becomes  red 

(See  Chromium 

yields   a   me 

dish  and  on 

reaction.) 

tallic   button. 

cooling  pale 

grey. 

As  pyromor- 

Dissolves  rea 

As  in  borax. 

Yields  metallic 

Fused  as  above 

phite. 

dily  and  gives 

lead. 

with  K,S2 

the  molybdena 

forms  a  yellow 

reaction. 

mass,  which 

becomes  white 

on  cooling.  If 

this  be   dis 

solved  in  water 

and  a  piece 

of  zinc  intro 

duced  into  the 

> 

solution,   the 

latter  becomes 

\ 

blue. 

246 


BEHAVIOK     OF     MINERALS 

LEAD.     (Continuation  of  page  245.) 


Mineral. 

Formula. 

Behavior 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

Scheeletine  .  .  . 

4 

PbW. 

Decrepitates 
more  or  less. 

Fuses  to  a 
bead  incrust- 
ing  the  char 
coal  with  PbO. 
The  bead  on 
cooling  is  crys 
talline  and  has 
a  dark  metal 
lic  surface. 

BEFORE    THE     BLOWPIPE.  247 

LEAD.     (Continuation  of  page  246.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

w 

with  carb.  soda. 

As  pyromor- 
phite. 

Dissolves  to  a 
clear  colorless 
glass,  which  in 
the  reducing 
flame  becomes 
yellow,  and  on 
cooling   grey 
and  opaque. 

Dissolves  to  a 
clear  colorless 
glass,  which  in 
the    reducing 
flame  assumes 
a  dusky  blue 
color.  After  a 
time  becomes 
opaque. 

As  the  pre 
ceding. 

With  carbo 
nate  of  soda 
and  nitre  gives 
the  manganese 
reaction. 

24:8  BEHAVIOR    OF    MINERALS 

COPPER. 


Minpral 

] 

5  e  h  a  v  i  o 

r 

«>.ll  I  ICI  Ori» 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

Xative  copper 

Cu 

_ 

_ 

Fuses  to  a 

brilliant  me 

tallic  bead, 

which  on  cool 

ing  becomes 

covered  with 

a  coating  of 

black  oxide. 

Vitreous   cop- 

Cu3S. 

Evolves  SO2 

Fuses  to  a 

and   when  pul 

bead   which 

verized  and 

spirts   consi 

gently  heated 

derably  and 

for  some  time 

gives  off  SO2. 

is  converted 

When  pulver 

into  CuO. 

ized  and  gently 

roasted,  is  con 

verted  into 

CuO. 

Copper  pyrites 

€uFe. 

Decrepitates, 
sometimes 

Evolves  SO2 
and  is  finally 

Fuses  readily 
with    much    j 

gives  a  subli 

converted  into 

ebullition  and 

mate  of  sulphur 

a   dark   red 

is   magnetic 

and   becomes 

mixture  of 

on  cooling. 

bronze  colored 

Fe20b  and 

on  the  surface. 

CuO. 

BEFOKE    THE     BLOWPIPE.  249 

COPPER.     (Continuation  of  page  248.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

(?) 

with  carb.  soda. 

Fuses  and  co 

In  the  oxidiz 

As  in  borax. 





lors  the  outer 

ing  flame  dis 

flame  blue. 

solves  and  then 

gives  the  cop 

per  reactions. 

The  roasted 

As  in  borax. 

In  the  reduc 

mineral  gives 

ing  flame  is 

the  copper  re 
action,    and 

decomposed, 
forming   NaS 

sometimes 

and  metallic 

also  a  slight 

copper.    If  the 

iron-reaction. 

former  be  cut 

out  and  laid 

upon  silver,  it 

gives  the  sul 

phur  reaction. 

As   the  pre 

As   the  pre 

Yields  a  bead 

_ 

ceding  ;    but 

ceding,   but 

of  metallic 

when  the  cop 

the  color  in 

copper  and 

per  has  been 

the  oxidizing 

some  magnetic 

removed  by 

flame  is  green, 

oxide  of  iron, 

reducing  on 
charcoal,   the 

owing  to  the 
presence  of 

which  remains 
on  the   char 

bead  shows  a 

iron. 

coal.      The 

strong  iron 

fused   alkali 

color. 

gives  a  sul 

phur  reaction 

on  silver. 

- 

11* 


250 


BEHAVIOR    OF     MINERALS 


COPPER.     (Continuation  of  page  249.) 


•»!••..      -1 

3 

3  e  h  a  v  i  o 

r 

Mineral. 

JL  orniulii. 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 

on  charcoal. 

Fahlerz      .... 

(<3uAgFeZn)4 

Sometimes 

Fuses  and  gives 

Fuses  to  a 

(SbAs). 

decrepitates, 
fuses,  and  when 

off  thick  fumes 
of  SbO3  and 

bead,  which 
fumes  strongly 

very  strongly 

SO2,  also  gene 

and   incrusts 

heated,  gives  a 

rally  AsO3, 

the   charcoal 

red  sublimate 

leaving  a  black 

with  SbO3, 

of'SbwithSb, 

infusible  resi 
due       If  Hg 

and  sometimes 
ZnO,  which 

also  sometimes 
a  black  subli 

be  present,  it 

is  sublimed  and 

cannot  be 
volatilized. 

mate  of  Hg 

condenses  in 
the   tube  in 

Emits  a  strong 
smell   of 

and  occasion 

small  drops. 

arsenic. 

ally  As. 

Tennantite  .  .  . 

(€uFe)4As. 

Decrepitates 
occasionally 

Evolves  S  and 
A*s,  which  con 

Fuses  to  a 
magnetic  bead 

and  gives  a 

dense  and  form 

giving  off  ar 

red  sublimate 

a  white  subli 

senical  and 

in 

of  As. 

mate. 

sulphurous 
fumes. 

Bournonite  .  .  . 

(Pb2<3u)Sb. 

Decrepitates 

Evolves  thick 

Fuses  readily 

giving  off  sul- 

white  fumes  of 

and    incrusts 

3hur  and,  when 

.. 

the  charcoal 

strongly  heat 

3b,Sb  and 

with  Sb  and 

ed,  Sb  and  Sb. 

Pb§b.    Also  S. 

Pb  leaving  a 
dark  colored 

bead. 

BEFORE    THE    BLOWPIPE.  251 

COPPER.     (Continuation  of  page  250.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

CO 
with  carb.  soda 

_ 

The  residue 

As  the  pre 

With  this  flux 

If  the  copper 

obtained  on 

ceding. 

and  a  little 

bead  obtained 

charcoal  thor 

borax  yields  a 

by  fusing  upon 

oughly  roaste( 

bead  of  metal 

carbonate  of 

gives  a  copper 

lic  copper  ;  on 

soda  be  cupel 

reaction,  and 

silver,  the  al 

led  with  assay 

when  the  lat 

kaline  mass 

lead,  a  silver 

ter  has  been 

gives  a  sul 

bead  will   be 

removed  by 

phur  reaction. 

obtained.  Or  if 

reduction  upon 

dissolved  in  ni 

charcoal,   an 

tric  acid  and  a 

iron  reaction. 

drop  or  two  of 

HCC1  added,  a 

white  precipi 

tate  of  AgCl 

will  be  formed, 

which  may  be 

collected  and 

reduced  with 

carbonate  soda 

upon  charcoal. 

__ 

As  the   pre 

As   the   pre 

Yields  a  copper 



ceding. 

ceding. 

bead  and  metal 

lic  iron  in  the 

form  of  a  dark 

grey  powder. 

The  fused  alkali 

gives  the  sul 

phur  reaction. 

__ 

If  the  bead 

As  with  borax. 

Yields  a  bead 



obtained  on 

of  metallic  cop 

charcoal  be 

per  and  lead 

fused  on  that 

and   incrusts 

support  in  the 
reducing  flame 

the  charcoal 
with  Sb  and 

with  borax,  a 

Pb.  The  alka 

light  iron  reac 

line  mass  laid 

tion  is  obtain 

on  silver  and 

ed,  and  after  a 

moistened 

time  a  copper 

gives  the  sul 

reaction. 

phur  reaction. 

252 


BEHAVIOB     OF     MINERALS 


COPPER,     (Continuation  of  page  251.) 


Formula. 

I 

J  e  h  a  v  i  o 

r 

Mineral. 

CD 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

lied   oxide  of 

Cu20. 

_ 

Is  converted 

In  the  re  due- 

copper 

into  ttiG  bl&ck 

*              fl 

oxide  CuO. 

reduced,  form 

ing  a  bead  of 

metallic  cop 

per. 

Atacamite  .... 

CuCl-}-3Cu 

Gives  off  much 



Fuses,  colors 

4-6^ 

water,  having 

the  flame  blue, 

an  acid  reac 

forms  a  brown 

tion,   on   test 

and   a   pale 

paper,   and 

grey  incrusta 

forms  a  light 

tion   on   the 

grey  sublimate 

charcoal,  and 

of  CuCl. 

is  reduced  to 

metallic   cop 

per,  leaving  a 

small  quantity 

of  slag. 

Dioptase  ..... 

Cu3Sia+3fl. 

Gives  off  water 

_ 

In  the  oxidiz 

and   turns 

ing  flame  be 

black. 

comes   black. 

In  the  reduc 

ing  flame  red. 

Malachite  

Gives  off  water 

Fuses   to  a 

and   turns 

bead  and  with 

black. 

a  strong  flame 

is  reduced  to 

metallic  cop 

per. 

BEFORE     THE     BLOWPIPE.  253 

COPPER.     (Continuation  of  page  252.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
iu  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

(?) 

with  carb  soda. 

Fuses  and  co 
lors  the  flame 

Gives  the  cop 
per  reaction. 

As  with  borax. 

Is  reduced  to 
a  bead  of  me 

— 

emerald  green, 

tallic  copper. 

or  if  previously 

moistened 

with  HC1,  blue. 

Fuses  and  co 
lors  the  outer 

Gives  the  cop 
per  reactions. 

As  with  borax. 

Is  reduced, 
yielding  a  bead 

— 

j  flame  intensely 

of  metallic 

blue  and  green 

copper. 

towards  the 

point. 

V. 

Gives  the  cop 

As  with  borax. 

With  a  small 

Colors  the 

per  reactions. 

The  silica  re 

quantity  of 

outer  flame 

mains    undis- 

carbonate  of 

intensely 

solved. 

soda  fuses  to 

green. 

a  bead,  which 

on  cooling  is 

opaque  and 

has  a  red  frac 

ture.     With 

more    alkali 

forms  a  slag, 

containing 

little  beads  of 

reduced   cop 

per. 

Fuses  and  co 
lors  the  outer 

Gives  the  cop 
per  reaction. 

As  in  borax. 

Yields  metal 
lic  copper. 

Dissolves  in 
HC1  with  much 

,  Ihune  brilliant 

effervescence. 

ly  green. 

254: 


BEHAVIOR     OF    MINERALS 


COPPER.     (Continuation  of  page  253.) 


I 

Behavior 

Mineral. 

Formula. 

(1) 

in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

Blue  vitriol.  .  .  . 

Cu§-f5S. 

Intumesces, 

Strongly  heat 

As  in  the  glass- 

gives  off  water 
and  becomes 
white. 

ed  is  decom 
posed,  giving 
off  SO2  and 

bulb.     Then 
fuses,  coloring 
the  outer  flame 

being  convert 
ed  into  CuO. 

green,  and  is 
reduced  to  me 

tallic    copper 

and  €u. 

Libethenite  .  .  . 

Cu4P"+2H. 

Gives  off  water 



Gradually  heat 

and    turns 

ed,  turns  black 

black. 

and  fuses  to  a 

bead,  having  a. 

core  of  metal 

lic  copper. 

Olivenite 

Cu4(ls5>)+fl. 

Gives  off  water. 

Fuses  with  de 

tonation   and 

the  evolution 

of  arsenical 

fumes  to  a 

brittle  regu- 

lus,  brown  ex 

ternally  and 

having  a  white 

fracture. 

BEFORE    THE    BLOWPIPE.  255 

COPPER.     (Continuation  of  page  254.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

(V) 
with  carb.  soda. 

Fuses  and  co 

The  roasted 

As  in  borax. 

Yields  metal- 

Gives  the  sul 

lors  the  outer 
flame  blue. 

mineral  gives 
the  copper 

ic  copper.  The 
alkaline  mass 

phuric   acid 
reaction. 

reaction. 

laid  on  silver 

gives  the   S 

reaction. 

Fuses,  but  does 
not  color  the 
flame  distinct 

Gives  the  cop 
per  reaction. 

A.S  in  borax. 

With  much  of 
the   alkali    is 
decomposed, 

Gives  the  phos 
phoric   acid 
reaction. 

ly.  On  cooling 

yielding  me 

is   black  and 

tallic  copper. 

crystalline. 

With    small 

portions   suc 

cessively  add 

ed  first  fuses 

and  then   in- 

tumesces,  fuses 

with  a  strong 

flame,  and  is 

then  absorbed 

into  the  char 

coal,    leaving 

metallic   cop 

per. 

Fuses  and  co 

Gives  a  copper 

As  in  borax. 

Is   reduced, 

Gives  the  arse 

lors  the  outer 

reaction. 

yielding  me 

nic  reactions. 

flame  green. 

tallic  copper. 

On  cooling  has 

a  crystalline 

surface. 

256 


BEHAVIOR     OF     MINERALS 
ANTIMONY. 


] 

3  e  h  a  v  i  o 

p 

All  11C  Tell. 

TPonniilfl, 

(i) 

(2) 

(3) 

in  glass-bulb. 

in  open  tube. 

on  charcoal. 

Native   anti- 

Sb. 

Fuses  and, 

Fuses  and  gives 

Fuses  and  gives 

when  strongly 

off  dense  white 

off  dense  white 

heated,  volati 

fumes,  which 

fumes,  which 

lizes  being  re- 

are  partly  re- 

thickly  incrust 

deposited   in 

deposited    on 

the  charcoal 

the  tube  as  a 

the  tube. 

and  color  the 

dark  grey  sub 

Sometimes  also 

blame    blue 

limate. 

gives  oif  arse 

immediately 

nical  fumes  in 

beyond   the 

small  quantity. 

assay. 

Grey  antimony 

SbS3. 

Fuses  readily 

Fuses  and  gives 

Fuses   and  is 

and  occasion 

off  SO2,  which 

partly  absorb 

ally  gives  off 

passes  off  up 

ed    by  the 

a  small  quan 

the  tube,  and 

charcoal   and 

tity  of  sulphur. 

dense  white 

partly  volati 

Strongly  heat 

fumes   of 

lized,  incrust- 

ed    forms    a 

SbO3  and  SbO5, 

ing  the  char 

brown  subli 

which   are 

coal  with  the 

mate  of  SbS3 

partly  deposit 

characteristic 

and  SbO3. 

ed  in  the  tube. 

white  oxides. 

Colors    the 

flame  blue. 

Antimony 
blende  

3b«+Sb. 

Fuses    easily, 
gives  off  first 

As  the   pre 
ceding. 

As  the  pre 
ceding. 

SbO3  and  af 

terwards    an 

orange  colored 

sublimate. 

Strongly  heat 

ed,  is  decom 

posed  and  gives 

a  black  subli 

mate,   which 

becomes  brown 

on  cooling. 

B  E  F  o  K  E    TUB    BLOWPIPE.  257 

ANTIMONY.     (Continuation  of  page  256.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

(?) 
with  carb.  soda. 

The  oxide 

As  in  borax. 

The  incrusta 

formed    upon 

tion  on  the 

charcoal  gives 

charcoal,    if 

the  antimony 

treated  with 

reactions. 

nitrate  of  co 

balt  assumes 

the  character 

istic  green 

color. 

— 

As  the   pre 
ceding. 

As  in  borax. 

Fuses  and   is 
reduced,  yield 
ing  metallic 

As  the   pre 
ceding. 

antimony, 

which  behaves 

as  the  preced 

ing   mineral 

upon  charcoal. 

The  alkaline 

mass  gives 

the  sulphur 

reaction. 

As  native 

As  in  borax. 

As  the   pre 

As  native 

antimony. 

ceding. 

antimony. 

258 


BEHAVIOR    OF     MINERALS 

ANTIMONY.     (Continuation  of  page  257.) 


J 

3  e  h  a  v  i  o 

r 

Mineral. 

Formula. 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

White   anti 
mony  .        . 

SbO3. 

Is  sublimed 
and   recon- 

As  in  the  glass- 
bulb. 

Fuses  with  the 
evolution   of 

densed  in  the 
neck  of  the 
tube. 

dense  white 
fumes,  which 
incrust    the 
surface  of  the 
charcoal.     In 
the   reducing 
flame  is  partly 
reduced,  yield 
ing  metallic 
antimony. 
Colors  flame 
blue. 

BEFORE    THE     BLOWPIPE.  259 

ANTIMONY.     (Continuation  of  page  258.) 


Behavior 

(8) 

(4) 

(5) 

(6) 

(V) 

reactions. 

in  forceps. 

in  borax. 

in  mic.  salt. 

with  carb.  soda. 

Fuses  and  is 
volatilized, 
coloring  the 
outer  flame 

Gives    the 
antimony 
reaction. 

As  in  borax. 

In  the  reduc 
ing  flame  is 
reduced,  yield 
ing    metallic 

As  native 
antimony. 

blue. 

antimony. 

.-     •;   .  >      ,.».    -/.. 

260  BEHAVIOK     OF     MINERALS 

ARSENIC. 


Mineral. 

I 

5  e  h  a  v  i  o  i 

Jb  orniuui. 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

Native  arsenic 

As. 

Sublimes  with 

If  gently  heat 

Passes  off  as 

out  fusion  and 

ed  in  a  good 

AsO3,  which 

recondenses  as 

current  of  air 

thinly  incrusts 

a  dark  grey 

passes  off  as 

the  charcoal 

metallic  sub 

AsO3,  which 

beyond  the 

limate,  some 

is  partly  con 

assay. 

times  leaving 

densed    as    a 

a  small  residue. 

white   subli 

mate  in  the 

upper  part  of 

the  tube. 

AsS2. 

Fuses,  enters 

Gently  heated 

Fuses  and 

into  ebullition 

passes  off  as 

passes  off  as 

and   is   sub 

SO2  and  AsO3, 

arsenious  and 

limed    as    a 

the  latter  of 

sulphurous 

transparent 

which  is  rede- 

acids. 

red  sublimate. 

posited  in  the 

upper  part  of 

the  tube. 

Orpiment  

AsS3. 

As  the   pre 
ceding,  except 

As   the  pre 
ceding. 

As  the  pre 
ceding. 

that  the  sub 

limate  is  of  a 

dark   yellow 

color   when 

cold. 

White  arsenic 

AsO3. 

Sublimes  with 

_ 

Sublimes  and 

out  fusion  and 

is    partly   re- 

recondenses  in 

condensed  on 

white  crystals. 

charcoal  form 

ing   a   white 

incrustation. 

B  E  F  o  it  E    THE    BLOWPIPE.  261 

ARSEXIC.     (Continuation  of  page  260.) 


Behavior 

(8) 
Special 
reactions. 

(*) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

en 

with  carb.  soda. 

Colors  the 

_ 

_ 



flame   blue. 

Fuses  and  co 

As   on   char 

lors  the  flame 

coal,   except 

blue. 

that    the   S 

combines  with 

the  alkali 

forming  NaS, 

which  on  sil 

ver  gives  the 

sulphur  reac 

tion. 

As  the  pre 
ceding. 

—  • 

— 

As  the   pre 
ceding. 

— 

Colors  the 

Heated  with 

flame  blue. 

charcoal  in  a 

glass-tube 

sealed  at  one 

end,  is  reduced 

and  metallic 

arsenic  sub 

limes 

262  BEHAVIOR    OF     MINERALS 

MERCURY. 


ITnrmiila 

] 

B  e  h  a  v  i  o 

r 

Jiliiior3.1» 

C  UI  mulct. 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 

on  charcoal. 

Native  mercury 

Hg. 

Volatilizes  with 

_ 

Is  volatilized. 

little    or  no 

residue  and 

recondenses  in 

neck  of  bulb. 

Cinnabar      .  .  . 

HffS. 

Volatilizes 

If  gently  heat 

Is  volatilized 

-1-l.gKJ. 

sometimes 

ed  is  decom 

generally  leav 

ieaving  a  sligh 

posed    into 

ing   a  small 

earthy  residue, 

metallic  mer 

earthy  residue. 

and   recon 

cury,  which 

denses  as  a 

volatilizes  and 

3lack  sulphide 

recondenses 

in  the  upper 

part  of  the 

tube,  and  SO2, 

which  passes 

off  and  is 

easily  recog 

nized  by  its 

odor  and 

teaching  pro 

perties. 

Native    amal- 

AgHg2. 

As  native 
mercury,  but 

— 

The  mercury 
volatilizes 

leaves  a  resi 

leaving  the 

due  of  pure 

silver,  which 

silver. 

fuses  to  a 

bead,  and,  in 

the  oxidizing 

flame,  incrusts 

the  charcoal 

with  its  cha- 

racteri  sti  ^ 

oxide. 

B  E  F  o  it  E    THE     BLOWPIPE.  263 

MERCURY.     (Continuation  of  page  262.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

(V) 
with  carb.  soda. 

With  carbo 

When  in  the 

nate  of  soda 

preceding  ex 

and  cyanide 
of  potassium 
is  decomposed 
and  metallic 

periment   the 
mercury  has 
been  entirely 
dissipated,  the 

mercury  vola 

alkaline   resi 

tilized. 

due   laid   on 

1 

silver  gives  a 

sulphur  reac 

tion. 

1 

• 

264:  BEHAVIOR     OF     MINERALS 

SILVER. 


Mineral. 

Formula. 

] 

3  e  h  a  v  i  o 

r 

(1) 
in  glass-bulb. 

(2) 
in  open  tube. 

(3) 
on  charcoal. 

i 

Native  silver.  . 

Ag- 

_ 

_ 

Fuses  and  in 

a  strong  oxi 

dizing   flame 

forms   an  in 

crustation   of 

dark   brown 

oxide  on  the 

charcoal.     If 

any  antimony 

be  present,  it- 

affords  a  crim 

son   incrusta 

tion. 

Antimonial 

Gives  off  dense 

Fuses,    fumes 

silver  

Ag'Sb. 

white    fumes 

strongly,  form 

which   are 

ing   a    white 

partly  deposit 
ed  in  the  tube. 

incrustation, 
and  when  the 

antimony  is    j 

nearly  expelled^ 

a  crimson  one, 

a  nearly  pure 

silver    bead 

remains. 

Silver  glance.  . 

AgS. 

— 

Gives  off  sul 
phurous  acid. 

Gives  off  SO'2 
and  is  reduced 

to  metallic  sil 

ver.  If  impure, 

a  small  quan 

tity   of  slag 

also  remains. 

| 

BEFORE     THE     BLOWPIPE.  265 

SILVER.     (Continuation  of  page  264.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

(?) 

with  carb.  soda. 

Gives  the  sil 
ver  reactions. 

As  in  borax. 

— 

The  incrusta 
tion  formed 
on  charcoal 
gives  an  anti 
mony  reaction. 

As  in  borax. 

As   alone    on 
charcoal. 

— 

— 

The  residual 
slag  (if  any) 
obtained  upon 
charcoal  gives 
an  iron  reac 
tion. 

As  in  borax. 

As  alone   on 
charcoal.   The 
alkaline  mass 
gives  a  sulphur 
reaction   on 
polished  silver. 

12 


266 


BEHA.VIOK    OF    MINERALS 


SILVER.     (Continuation  of  page  265.) 


Mineral. 

Formula. 

Behavior 

(1) 

(2) 

(8) 

in  glass-bulb. 

in  open  tube. 

on  charcoal. 

Stephanite  .... 

AgsSb. 

Decrepitates, 
fuses  and  gives 

Fuses  and     i 
gives  off  SO2  i 

Fuses  and  in- 
erusts  the  eha- 

i  a  slight  subli 

and  dense     icoal  with  anti- 

mate   of   sul 

white  antimo 

monious  acid, 

phide  of  anti- 

nial  fumes. 

leaving    Ag 

mouy. 

with  some  an 

timony.      If 

the  flame  be 

continued,    a 

red    iuerusta-  i 

tion  is  formed 

I  and  finally  a  . 

bead  of  pure 

silver  remains 

surrounded  by 

a  small  slag. 

Pyrargyrite  .  .  . 

Ag3Sb. 

Sometimes 
decrepitates, 

As   the   pre 
ceding. 

Fuses  with 
much  spirting 

fuses  readily, 

and  covers  the 

and,  when 

charcoal  with 

j  strongly  heat-                                   antimonial 

ed,  gives  a   j 

fumes.  When 

dark  red  sub- 

the   residual 

limate  of  SbSa. 

AgS  is  heated 

for  some  time 

in  the  oxidiz 

ing    flame,    a 

bead  of  pure 

silver  is  ob 

tained. 

Proustite  

Ag8As. 

Fuses  and  at 

Gradually  heat- 

As   the   pre- 

!  a  low  red  heat    ed  it  gives  oft'   ceding,  except 

affords  a  small     AsO3  and  SO*,     that   a   large 

sublimate   of    Sometimes  also;    quantity    of 

AsS3. 

antimony 

AsO  and  but 

fumes. 

little  SbO3  are 

given   off. 

1 

BEFORE    THE    BLOWPIPE.  267 

SILVER.     (Continuation  of  page  2CG.) 


Behavior 

(8) 
Special 
reactions. 

(4) 
in  forceps. 

(5) 
in  borax. 

(6) 
in  mic.  salt. 

(*) 

with  carb.  soda. 

The  residual 

As  in  borax. 

The  silver  is 

slag  obtained 

reduced    and 

on   the  char 
coal  gives  an 

the  antimony 
passes   off  in 

iron  and  cop 

dense  fumes. 

per  reaction. 

The  fused  al 

kali  gives  the 

sulphur-reac 

tion  on  silver. 

As   the   pre 

ceding. 

• 

As  stephanite, 

except   that 

much  arsenic 

i   is   given   off 

and  but  little 

antimony. 

268 


BEHAVIOR    OF     MINERALS 

SILVER.     (Continuation  of  page  267.) 


Behavior 

Mineral. 

Formula. 

(1) 

(2) 

(3) 

in  glass-bulb. 

in  open  tube. 

on  charcoal. 

Horn  silver  .  .  . 

AgCl. 

Fuses,  but  un 

_ 

Fuses  readily 

dergoes    no 

in  the  oxidiz 

further  change. 

ing  flame.    In 

the   reducing 
flame  is  slowly 

reduced  yield 

ing  metallic 

silver. 

BEFORE    THE     BLOWPIPE.  2C9 

SILVER.    (Continuation  of  page  268.) 


Behavior 

(8) 

^snppinl 

(4) 

(5) 

(6) 

en 

opcClal 

reactions. 

in  forceps. 

in  borax. 

in  mic.  salt. 

with  carb.  soda. 

_ 

_ 

_ 

Is  rapidly  re 

If  cut  up  into 

duced  to  me 

small   pieces 

tallic  silver. 

mixed   with 

oxide  of  cop 

per  and  then 

heated  before 

the  oxidizing 

flame    upon 

charcoal,    it 

colors    the 

flame  blue. 

THE   END, 


H.    B  A.  ILL  IE  RE'S 

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Use  of  the  Blowpipe,  translated  by  Children.    Svo.    London.    (Very  scarce.) 

Traite  de  Chimie.    Nouv.  edit.,  par  B.Valerius.    4  vols.,  gr.  8vo.,  avec  S  planches. 

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Blancli imeiit.  Nouveau  Manuel  complet  du  Blanchiment,  du  Blanchissage,  Nettoyage 
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Black  (W.)    Practical  Treatise  on  Brewing.    4th  edit.    Svo.    London,  1849    .  .    8  25 

Blanquart  (Evrard.)    Traite  de  Photographic  sur  Papier.    Svo.    Paris.  1851  .    1  25 

Blowpipe.    See  SANDERS,  Dr.  J.  M. 

Boucliardat*    Opuscules  d'Economie  Rurale.    Svo.    Paris,  1851       .         •    »    •          .    1  00 

Bouquet  ( J.  P.)  Histoire  Chimique  des  Eaux  Minerales  et  Thermales  de  Vichy.  Cusset, 
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Chateldon,  Brugheas  et  Seuillet.  8vo.,  8  cartes.  Paris,  1855  .',•._  •  .175 

Bo  ussingault.  Rural  Economy ;  in  its  Relations  with  Chemistry,  Physics,  and  Meteor 
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Boutigny.    Base  d'une  Nouvelle  Physique,  1'etat  Spheroidal.    Svo.    1842       .     ,     ••!• 

Bowman  (J.  E.)    Introduction  to  Practical  Chemistry.    2d  edit.    12mo.     '.-/ 

Brande.    Tables  of  Chemical  Equivalents.    Svo.    London     .  .         ,    \ 

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epreuves  instantanees ;  traite  complet  des  divers  precedes.    8vo.     Paris,  1852  .  .    1  00 

Traite  Complet  de  Photographic  sur  Collodion  ;  repertoire  de  la  plupart  dea  Pro- 
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Brown  (A.)     The  Philosophy  of  Physics,  or  Process  of  Creative  Development.    8vo. 

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Chevalier.  Recueil  de  Memoires  et  de  precedes  nouveaux  contenant  la  Photographic 

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Chevalier  (C.)  Photographic  sur  Papier,  Verre,  et  Metal.  Galvanoplastie.  Catalogue 

universel    explicatif  et  illustre  des  appareils  perfectionnes.     Svo.,  avec  3  planches. 

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Chevallier.  Dictionnaire  des  Alterations  et  Falsifications  des  Substances  Alimentaires, 

Medicamenteu«es  et  Coimnerciales,  avec  1'Indication  des  Moyens  de  les  Reconnaitre. 

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Chevallier,  Lamy.  and  Kobiquet.  Dictionnaire  raisonne  des  denominations 

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2me  edit.,  tome  ler.  Paris,  1858 .  "  ..  i  .  .  .  .  .225 

Chevreul.  De  la  Baguette  divinatoire,  du  Pendule,  dit  Explorateur,  et  des  Tables  Tour- 

nantes,  au  point  de  vue  d'Histoire,  de  la  Critique  et  de  la  Methode  Experimental*,    Svo. 

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Atlas.     Paris,  1889          ........ 

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C  Jaudet.    Nouvelles  Recherches  sur  la  difference  entre  les  Foyers  Visuels  et  Photogeniques. 

8vo.    Paris,  1851  .  .  .  -.  .  .  .  .050 


Treatise  on  the  Manufacture  of  Coal  Gas.  4to.  London  .  .  .  8  87 

Codex*  Pharmacopee  Francaise,  redigee  par  ordre  du  gouvernement,  avec  appendice 

therapeutique,  par  Cazenave.    8vo.    Paris,  1837     .  .  .  .  .    2  50 

In  half  calf   .  .  .  .  .  .  .  .  .    8  00 

Coloriste.  Nouveau  Manuel  Complet  du  Coloriste,  ou  Instructions  Simplifiees  et  elemen- 

taires  pour  l'enluminure,le  lavis  etla  retouche  des  gravures.    Nouvelle  edition.    18mo., 

avec  3  planches.  Paris,  1856  .  .  .  .  P  .  0  75 

Colles.  Nouveau  Manuel  de  la  Fabrication  des  Colles,  comprenant  la  Fabrication  des 

Colles  de  Matieres  Vegetales,  par  M.  Malpeyre.  12mo.  Paris,  1856  .  .  .  0  50 

Cooley  (A.  J.)  Cyclopedia  of  Practical  Receipts,  and  collateral  information  in  the  Arts. 

Manufactures,  Professions,  and  Trades;  including  Medicine,  Pharmacy,  and  Domestic 

Economy  ;  designed  as  a  comprehensive  supplement  to  the  Pharmacopoeia,  and  general 

book  of  reference  for  the  Manufacturer,  Tradesman,  Amateur,  and  heads  of  Families. 

3rd  edition.    8vo.    London,  1S56  .  .  .  .  .  .    8  00 

Cooper  (C.)  Identities  of  Light  and  Heat  ;  of  Caloric  and  Electricity.  8vo.  Philadel 

phia,  1S43         .  ....  .    0  T5 

Cotte.     Observations  Meteorologiques.    4to.  .  .  .  .  .    0  60 

Coulomb*  Methode  de  determiner  1'Inclinaison  d'une  Aiguille  Aimantee.  4to.  .  0  25 

Crabb  (G.  A.)  Technical  Dictionary  ;  or  a  Dictionary  explaining  the  terms  used  in  all 

Arts  and  Sciences.  12mo.  London,  1851  .  .  .  .  .375 

dimming,  J.  A  Manual  of  Electro  Dynamics.  Svo.  London,  1827  .  .  1  50 

Clindall  (  J.)  The  Photographic  Primer  for  the  use  of  beginners  in  the  Collodion  process. 

Illustrated  with  a  Photographic  Picture.  2d  edit.  12mo.  London,  1856  .  .  0  31 

Cuvier.  Analyse  de  ses  Travaux  sur  la  Physique  et  la  Chimie.  4to.  .  .  .  0  60 

Daguin  (P.  A.)  Traite  Elementaire  de  Physique  Theorique  et  Experimentale,  avec  les 

Applications  a  la  Meteorologie  et  aux  Arts  Industriels.     Tome  ler.    Avec  300  gravures 

sur  bois  intercalees  dans  le  texte.  Svo.  Paris,  1856  .  .  .  .  3  00 

Dal  ton  (John),  Life  and  Scientific  Researches  of.  ByW.  C.Henry.  Svo.  London,  1854  3  50 

-  Chemical  Philosophy.    2  vols.,  Svo.    London  .  ..  .  .    9  50 
Daniel  I  (  J.  F.)    An  Introduction  to  the  Study  of  Chemical  Philosophy  ;  being  a  prepa-    8  00 

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edition.    London,  1843     .  .  .  .  «  .  .  7  21 

Very  scarce. 
David.  (II.)    Methode  de  Peinture  appliquee  uniquement  a  la  Photographic  de  Portraits. 

2nd  edit.,  Svo.    Paris,  1856          .  .  .  .  .  .  .    0  50 

Davy  (Sir  H.)    Chemical  Philosophy.    Svo.     London          .         ;..*-.  .  .550 

--    Account  of  the  Safety  Lamp  for  Miners.    Svo.    London  .  .  .    1  50 

See  KNAPP'S  Technology. 
Delamotte  (P.)    The  Practice  of  Photography  :  a  Manual  for  Students  and  Amateurs. 

With  a  Calotype  Frontispiece.    3d  edition  revised.     12mo.     London,  1856        .  .    1  37 

-  The  Oxymel  Process  in  Photography.     12mo.    London,  1856     .  .  .    0  80 
De  la  Rive   (A.)      A  Treatise  on  Electricity  in  Theory  and  Practice.      2  vols.,  Svo. 

London,  1853-6  .  .  .  .  .  .  .  .  14  00 

-  --  (A.  —  A.)    Traite  d'Elec'ricite  Theorique  et  applique.    2  vol.,  Svo.,  avec  260  pi. 

intercalees  dans  le  texte.    Pari.*,  1853-1856       .  .  .  .  .45*) 

Les  nombreuses  applications  de  1'electricite  aux  sciences  et  aux  arts,  les  liens  qui  Tunis- 
sent  a  toutes  les  autres  parties  des  sciences  physiques,  ont  rendu  son  etude  indispen 
sable  au  chimiste  aussi  bien  qu'au  physicien,  au  geologue  autant  qu'au  physiologiste, 
a  1'ingenieur  comme  au  medecin;  tous  sont  appeles  a  rencontrer  1'electricite  sur  leur 
route,  tous  ont  besoin  de  se  familiariser  avec  son  etude.    Personne  mieux  que  M.  de 
la  Rive,  dont  le  nom  se  rattache  aux  progres  de  cette  belle  science,  ne  pouvait  pre 
senter  1'exposition   des   connaissances-  acquises  en  electricite  et  de  ses  nombreuses 
applications  aux  sciences  et  aux  arts. 
Desaiiis  (P.)     Legons  de  Physique,  a  1'Usage  des  Aspirants  aux  Baccalaureats  et  aux 

Ecoles  du  Uouvernement.    2  vols.     12mo.     Figures  intercalees  dans  le  texte     .  .     2  50 

Deschamps.     Art  (!')  de  Formuler,  contenant:    les  Principes  Elementaires  de  Phar- 

macie,  etc.     1  vol.,  19uio.,  avec  19  figures  intercalees  dans  le  texte.     Paris         .  .     1  2A 

DescloJzea  >x.      Memoir-!  sur  la  Cristallisation  et  la  Structure  Interieure  du  Quartz. 
8vo.,  plus  4  pi.     Paris,  1S56  ....... 

Deson^c.     Traite  de  Photographic  sur  Toile,  dernier  Perfectionnement.  Svo.    Paris,lS55    0  15 

Disdevi.  Manual  Operatoire  de  photographic  sur  collodion  instantane.  Svo.  Paris,  1S54  0  75 
--  Reiiseigueineuts  Photographiques  Indispensables  a  tous.  Svo.,  de  3  feuilles. 

P;tns,  1S55        .  .  r  .  .  .  .  .  .  .     1  2.5 

Dodd  (G.)  The  Curiosities  of  Industry  and  the  Applied  Sciences.  Svo.  Lon:lon,  1854  .  1  00 
Iiornr«,  Nouveau  Manuel  Complet  de  dorure  et  d'arsrenture  par  la  methode  e'<vtrr>- 

chifnique  et  par  simple  immersion  par  M.  M   Selmi.  de  Valecourt,  Malpeyre,  etc.    Nouv. 

edit  ,   tfL-s  auguientee,  ornee  de  figures.     !2mo.     Paris,  1S56  .  .    l»  50 

SI.  BieWiere,  29O  Xlroadway,  JV.   I". 


Standard  Scienli/lc    Works. 


Dove  (I?.  W.)  The  Distribution  of  Heat  over  the  Surface  of  the  Globe,  illustrated  by 
Isothermal,  Thermic  Isabnormal,  and  other  Curves  of  Temperature.  4to.,  with  map. 
London, 1853  .  I*  •  •  •  •  •  .  5  00 

Du   Bois-Ileymond  on  Animal  Electricity,  by  Bence  Jones.    8vo.    London,  1852    .    1  75 

Duhamel   de  Monceau.     Traite  de  la  Fabrique  des  Manoeuvres  pour  les  Vaisseaux 

ou  Tart  de  la  Corderie  perfectionne.    4to.     Paris,  1747  .  .  .  .    3  00 

Dubrunfaut.     Art  of  Distillation  and  Rectification.    12mo.    London.    (Very  Scarce)  . 
a.  ml  Koussingault.     The  Chemical  and  Physiological  Balance  of  Organic 

Nature:  an  Kssay.     12uio.  .  .  •  •  .  .  .     1  00 

Du  Moiicel  (Til.)   Projection  des  Principaux  Phenomenes  de  1'Optique  a  1'aide  des  ap- 

pareils  de  M.  Duboscq.     Svo.     Paris,  1855  .  .        50 
p:\pose  des  Applications  de  1'Electricite.     Tome  ler.     Notions  Technologiques  2me 

edit.,  8vo.,  avec  8  pi.    Paris,  1856.    (Cette  edition  aura  deux  vols  peut-etre  meme  trois)     \  25 
Dumas  (I.)    Essai  de  Statique  Chimique  des  Etres  Organises.    2ine  edit.    Paris,  1842    .    100 

Memoires  de  Chimie.    Avec  7  Planches.    Svo.     Paris,  1843        .  .  .     1  50 

Traite  de  Chimie  appliquee  aux  Arts.    8  vols.  and  4to  atlas.    Svo.    Paris,  1828-46. 

Very  scarce      .  .  .  .  .  •  •  .  .  50  00 

Edition  de  Bruxelles.    8  vols.  and  4to  atlas  .  .  .  .  30  00 

Dunn  (W.)    History  of  the  Steam  Jet  as  applicable  to  the  Ventilation  of  Coal  Mines.    Svo.    075 
I> u  plain  (P.)    Traite  des  Liqueurs  et  de  la  Distillation  des  Alcools,  ou  le  Liquoriste  et  le 

Distillateur  Modernes,  contenant,  etc.    2  vols.,  Svo.    Versailles,  1856  .  .  .    8  75 

Du  rand  (JPaug1.)    Nouvelle  Theorie  Physique  ou  Etudes  Analytiques  sur  la  Physique 

et  sur  les  actions  Chimique  fondamentales.    Svo.    Paris,  1S54  .  .  .75 

Encres.     Nouveau  Manuel  complet  de  la  Fabrication  des  Encres,  teUes  que  Encres  a 

Ecrire,  Chine,  de  Couleur  a  Marquer  le  Linge  &c.    18mo.    Paris,  1855  .  .    1  00 

Etoffes  Imprimees.     Nouveau  Manuel  Complet  du  fabricant  d'Etoffes  Imprimees  et 

du  Fabricant  des  papiers  peints,  par  L.  S.  le  Normand.    ISmo.    Paris,  1856      .  .        75 

Exhibition  of  1851  (Lectures  on  the  Results  of  the  Great,)  delivered  before  the 

Society  of  Arts,  Manufactures,  and  Commerce  (Dr.  Whewell,  Professor  Ansted,  and 

others).    2  vols.,  post  8vo.,  each  .  .  .  .  .  .  .    2  25 

Faraday  (JF.)    Chemical  Manipulations,  being  Instructions  to  Students  in  Chemistry. 

Svo.    London,  1827.    (Very  Scarce.)          .....       about    7  50 
Experimental  Researches  in  Electricity.    3  vols.,  Svo.    London,  1849-55.  .1350 

The  Subject-matter  of  a  Course  of  Six  Lectures  on  the  Non-metallic  Elements. 

12mo.,  cloth.    London,  1853,        .  .  .  .  .  .    1  75 

Fau  (JT.)    Douze  lecons  de  Photographic.    Description  de  precedes  simples  et  faciles,  au 
moyen  desquels  on  obtient,  presque  infailliblernent,  des  epreuves  sur  verre  et  papier.    • 
18rno.  .  .  .  .  .  .  .  .  .    0  75 

lya  it  et  Chevalier.    Manuel  du  Physicien  preparateur,  ou  description  d'un  cabinet  de 

Physique.    2  vols.,  ISmo.,  with  an  atlas  of  8S  plates.    Paris,  1853       .  .  .    8  75 

Faucher  (L«.)    Remarks  on  the  Production  of  the  Precious  Metals,  and  on  the  Demoniti- 

zation  of  Gold  in  Several  Countries  of  Europe.    Svo.    London,  1853,  .  .    0  75 

Faure  (J.  J.)  Analyse  Chimique  des  Eaux  du  departement  de  la  Gironde.  Svo.  Bor 
deaux,  1853  .  .  .  .  .  .  .  .  .  0  75 

Figuier  (I,.)    L'Alchimie  et  les  Alchimistes  ou  Essai  Historique  et  Critique  sur  la  Philo- 

sophie  llermetique.    2d  edit.    12mo.     Paris,  1856    .  .  .  .  .     1  00 

Fraiieceur  (Li.  B«)    Elements  de  Technologie  ou  Description  des  precedes  des  Arts.  Svo.    1  25 

1  railfis  (Ci.  IV.)  The  Dictionary  of  Practical  Receipts  ;  containing  the  Arcana  of  Trade 
and  Manufacture,  Domestic  Economy,  Pharmaceutical  and  Chemical  Preparations,  &c. 
Svo.  London,  1856  .  .  ,  .  .  .  .  2  50 

Frose  ill  us  (Dr.)    Instruction  in  Chemical  Analysis.    Quantitative.    2d  edit.   Svo.,  cloth. 

1S55  .  .  .  .  ...  .  .  .45:) 

Instructions  in  Chemical  Analysis.    Qualitative.    4th  edit.    Svo.,  cloth  .  .    2  75 

Fresenius  et  Sacc.     Precis  d'Analyse  Chimique  quantitative.     ISmo.     Paris,  1845. 

(Epuine.) 

Precis  d'Analyse  Chimique  qualitative.    1  vol.,  12mo.,  fig.    Paris,  1847.  (Epuiae.) 

Fyfe  (A.)    Elements  of  Chemistry.    Svo.    London    .  .  .  .  .    7  25 

Manual  of  Chemistry.    12mo.    London          .  .  .  .  .    2  12 

Galloway  (It.)    The  First  Step  in  Chemistry :  a  New  Method  for  Teaching  the  Elements 

of  the  Science.    2d  edit.    12mo.    London,  1855        .  .  .  .  .150 

Manual  of  Qualitative  Analysis.    12mo.,  cloth  .  .  .  .    1  12 

Chemical  Diagrams,  on  four  large  sheets        .'•  -  .  .  .  .    1  75 

Galvanoplastie.    Nouveau  Manuel  complet  de  Galvanoplastie,  ou  Elements  d'Electro- 

metallurgie;  contenant  1'Art  de  reduire  les  metaux  a  1'aide  du  tluide  sralvanique,  etc.,  par 
Smee.  Augmente  d'apres  MM.  Jacoby,  Spenctr.  Eisner,  etc.  Ouvrage  public  par  E.  de 
Valicourt.  2  vols.,  ISmo.  .  .  .  .  .  .  1  25 

II.  Hxillifrc,  29O  &ro€idway,  JIT.  JT, 


Standard  Scientific    Works. 


Oanot  (A.)  Traite  Elementaire  de  Physique  Experimentale  et  Appliquee,  et  de  Bletcoro- 
logie,  avec  un  recueil  nombreux  lie  problemcs,  illustre  de  5UO  gravures  sur  hois  inter- 
calees  dans  le  texte.  6e  edition,  auguientee  de  582  gravures  nouvelles.  ISmo.  Paris. 

1S56  .  .  ..ir; 

Gas.     Bvna  pp's  Chemical  Technology,  or  Chemistry  applied  to  the  Arts:  Fuel  and  its 

Application.     1vol.    In  2  Parts.     Stro.     London, 1 806  .  .  .  .    9  0« 

This  is  the  most  recent  and  complete  work  on  the  manufacture  of  Gas,  &c. 
Gas  L.i»-litiilg  (Journal  Of).    Published  in  London  on  the  10th  of  every  month. 

Price  per  year  .  .  .  .  .  .  .  .  .    8  11 

5  Vols.  are  published. 
Gaudiii  ( JI.  A.)    Traite  Pratique  de  Photographic,  expose  complet  des  precedes  rela- 

tife  au  Daguerreotype.    8vo.,  hf.  bd.  cf.     Paris,  1844  .  .  .  .    1  50 

Gauss  (C.  F1.)    Intensitas  vis  magnetica  terrestris  ad  mensuram  absolutum  revocata. 

4to.     Gottinga},  1833      .  .  .  .  .  .  .  .     1  5( 

Gavarret  ( J.)    De  la  Chaleur  produite  par  les  Etres  Vivants.    12mo.,  avec  41  figures 

dans  le  texte.     Paris,  1855  .  .  .  .  .  .  .     1  5C 

Gcrliardt.     Introduction  a  1'Etude  de  la  Chimie  par  le  Systeme  Unitaire.    12mo.    Paris, 

1S4S   .  .  .  .  .  .  .  .  .  .    1  0( 

• Precis  de  Chimie  Organique.    2  vjb..  Svo.     Paris,  1S44  .  .  .    4  (K 

In  half  calf  ...  .....    5  0( 

Traite  de  Chimie  Organique.    4  vols.,  Svo.    Paris,  1855-6  .  .  .  10  00 

Ce  Traite  est  une  suite  a  Berzelius.    Ce  celebre  chiiniste  etant  rnort  avant  d'avoir  pu 

terminer  son  ouvrage,  M.  Gerhardt,  ancien  professeur  de  chimie  a  Montpellier,  s'est 
charge  de  terminer  son  travail  et  de  le  mettre  au  courant  de  la  science  actuelle. 

Aide-memoire  pour  1' Analyse  Chimique.    12mo.    Paris,  1852     .  .  .    0  75 

Gerliardt  et  Chancel.    Precis  d'Analyse  Chimique.    12rno.,  avec  48  gravures.    Paris, 

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Glover  (R..  IH.)    A  Manual  of  Elementary  Chemistry :  being  a  Class-book.    Illustrated. 

12mo.     London,  1855     .  .  .  .  .  .  .  .    2  00 

Gmelin.     Handbook  of  Chemistry.    Vol.  1  to  6,  Inorganic  Chemistry  .  .  .  14  00 

"  Vol.  7  to  10,  Organic  Chemistry,  each  vol. .  .    4  50 

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nach,  1S50         .  .  .  .  .  .  .  .  .  10  00 

Gore  (G.)    Theory  and  Practice  of  Electro-Deposition,  including  every  known  mode  of 

depositing  metals,  etc.     Svo.     London,  1856  .  .  .  .  .    0  50 

Gorham.     Unfrequented  Paths  in  Optics.     Part  1.  Light  from  a  Pin-hole.    Part  2.  Light 

from  a  Fissure.     Svo.     London,  1855  .  .  .  .  .  .    1  25 

Graham.     Elements  of  Chemistry  ;  including  the  application  of  the  Science  in  the  Arts. 

By  T.  Graham,  F.R.S.  L.  &  E.,  Professor  of  Chemistry  at  University  College,  London. 

2d  edition,  entirely  revised  and  greatly  enlarged,  copiously  illustrated  with  Woodcuts. 

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• Vol.  2.    London  and  New  York,  185T  .  .  .  .  .    4  00 

This  work,  which  ranks  among  the  first  on  the  subject,  is  now  compltte. 

Chemical  Catechism.    Svo.    London  .  «  .  .  .    4  75 

Gregory  (Wm.)    Elementary  Treatise  on  Chemistry.    12mo.    Edinburgh,  1855  .    1  5j 
Handbook  of  Inorganic  Chemistry.    For  the  use  of  Students.    8d  edition.    12mo. 

London  .  .  .  .  .  .  .  .  .     i  75 

Handbook  of  Organic  Chemistry,  for  the  use  of  Students.    4th  edition,  corrected 

and  much  extended.    12mo.    London,  1S56  .  .  .  .  .    fc  62 

Griffin.     Treatise  on  the  Use  of  the  Blowpipe.    18mo.    London.    (Scarce.) 

Gritliii  (J.  J.)    Chemical  Recreation.    Div.  1,  post  Svo.        .  .  .  .    0  CO 

Griffith  (T.)     Chemistry  of  the  Four  Seasons.    12mo.    London,  1858  .  .  .225 

Grove  (W.  R.)    On  the  Correlation  of  Physical  Forces.    3d  edit.    Svo.    London,  1855  .    2  25 
Gruyer  (li.  A.)    Principes  de  Philosophic  Physique  pour  servir  de  base  a  la  Mctaphy- 

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Gilitoourt.     Histoire  naturelle  des  drogues  simples,  ou  Courg  '1'histoire  naturelle  professe 
a  1'Ecole  de  Pharmacie,  quatrieme  edition,  augmentee.    4  vo.  ,  8vo.,  avec  600  fig.  inter- 
calees  dans  le  texte.    Paris,  1S49  .  .  .  .  .  .    7  50 

Half  bound  in  Paris  .  .  .  .  .  .  .    9  50 

[Get  ouvrage,  que  tous  les  pharmaciens  considerent  comme  un  Vade-mecum  de  pre 
miere  necessite,  parce  que  la  grande  exactitude  apportee  par  1'auteur  dans  la  descrip 
tion  dea  drogues  leur  permet  de  distinguer  les  diverges  especes  et  varietes  qui  se  rencon- 
trent  dans  le  commerce,  ainsi  que  les  falsifications  qu'on  leur  fait  subir.  Cette  quatrieme 
edition  a  ete  soumise  a  une  revision  generate,  et  les  augmentations  ont  ete  tellement 
importantes,  qu'on  peut  la  considerer  comme  un  ouvrage  entierement  neuf.    C'est  un 
Cours  complet  d'kistoire  naturelle  pharmaceutique  et  medicale,  que  les  medecins 
consulteront  toujours  avec  fruit.] 
Guitard.    Histoire  de  1'Electricite.    12mo.    Paris,  1854          .  .  .  .    1  00 

Gumey.     Lectures  on  Chemistry.    8ro.    London     .  .  .  «,  ,    $  W 

U.  BaiUiere,  29O  ilrondiray,  .r.    *s. 


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Hardy  (12.  TV.  55.)  Incidental  Remarks  on  some  principles  of  Light ;  being  Part  8  of 

au  fcssay  ou  Vision.  8vo.  London,  1856  .  .  1  00 

llardwicli  (T.  I-'.)  A  Manual  of  Photographic  Chemistry,  including  the  Practice  of 

the  Collodion  Process.  2d  edition.  12ino,  cloth.  London  .  .  .  2  00 

Harris  (Stir  W.  S.)  Rudimentary  Treatise  on  Galvanism,  and  the  general  principles 

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13 a •* Mil  (  l.  11.)  Food  and  its  Adulterations.  With  159  illustrations.  8vo.  London, 

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He  atli.  Photography.  A  New  Treatise,  theoretical  and  practical,  of  the  Processes  and 

Manipulations  on  Paper  and  Glass.  Bvo.  New  York,  1855  .  .  .  .  1  00 

Hcdlt-y  (John).  Practical  Treatise  on  the  Working  and  Ventilation  of  Coal  Mines; 

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Kt  mi  all  (T.  M.)    The  Collodion  Process.    4th  edition.    12mo.    London,  1S55  .    0  &) 

Henry  (W.)    Elements  of  Experimental  Chemistry.    2  vols.,  Svo.    London      .  .  10  Hi 

Ilerling  (A.)    Traitede  Photographic  sur  Collodion  Sec.    2e  edition.    12mo.    Paris,  1856    050 

Itigliloii.     Treatise  on  the  Electric  Telegraph.    12mo.    London,  1852  .  .    0  60 

ItiutU  (l>r.  A*'.)  The  Harmonies  of  Physical  Science  in  relation  to  the  Higher  Senti 
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iloi-tcr  (2-'.)  Nomenclature  et  classification  chimiques,  suivies  d'un  lexique  historique  et 
synonymique  comprenant  les  noms  anciens,  les  formules,  les  noms  nouveaux,  le  nom  et 
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Paris,  1S45  .  .  .  .  .  .  .  .  0  75 

Hoefer.  Hist,  de  Chimie  depuis  les  temps  les  plus  recules  jusqu'a  nos jours.  2  vols.,  Svo. 
Paris,  1842.  (Very  scarce.)  ....... 

Hood  (C.)  A  Practical  Treatise  on  Warming  Buildings  by  Hot  Water,  on  Ventilation,  Ac. 

8d  edition.  Svo.  London,  1855  .  .  .  .  .  .  8  25 

Hopkins  (T.)  On  the  Atmospheric  Changes  which  produce  Rain  and  Wind.  2d  edit. 

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Hopkiuson  (J.)  The  Working  of  the  Steam  Engine  Explained  by  the  Use  of  the  Indi 
cator.  Svo.  London,  1854  .  .  .  .  .  .  .  1  50 

Horsfey  (J.  A.)  A  Catechism  of  Chemical  Philosophy;  being  a  familiar  exposition  of 

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Howard  (Luke.)    Seven  Lectures  on  Meteorology.    12mo.    London,  1848    .  .100 

Hewlett  (R.)  On  the  various  methods  of  Printing  Photographic  Pictures  upon  paper, 

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Hunt  (Robert).    Researches  on  Light.    Svo.    London,  1844  .  .  .    8  00 

Photography :  a  Treatise  on  the  Chemical  Changes  produced  by  Solar  Radiation, 

and  the  production  of  Pictures  from  Nature.    12mo.,  clo.    London    .  .  .    1  75 

Ellir*  aux.     Histoire  des  Falsifications  des  Substances  Alimentaires  et  Medicamenteuses, 
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Inorganic  Chemistry  (First  Outlines  of).    12mo.    London          .  .  .125 

Isadorc  G^offroy  Sainl-Hilaire.    Lettres  sur  les  Substances  Alimentaires  et  par- 

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\Vei<»bacli's  Mechanics  of  Machinery  and  Engineering.    Vols.  1  and  2,  with  900 

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Xt'cSinologry  t  or,  Chemistry  applied  to  the  Arts  and  to  Manufactures.    By  Drs. 

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Quekett's  Practical  Treatise  on  the  use  of  the  Microscope.    With  Steel  and  Wood 

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Fau's  Anatomy  of  the  External  Forms  of  Man.    For  Artists.    Edited  by  R.  Kuox, 

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Mitchell  (T.)    Manual  of  Practical  Assaying.    2d  edition,  much  enlarged.    Svo. 

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Johnson  (J,  F.  W.)    Instructions  for  the  Analysis  of  Soils,  Limestones,  and  Manures. 

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The  Chemistry  of  Common  Life.    2  vols.    12rao.    Edinburgh,  1855  .  .800 

II.  JBaillicrc,  29O  Broadway,  JT.  1". 


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Jourdaiu.    PlmrmacopeeUniverselle,  ou  Conspectus  de  toutes  les  Pharmacopees.  2vols. 

in-8.    2  edit.    Paris,  184U  .  .  .  .  •>.'"'          .  .    6  25 

Joyce  (Rev.  J.)    Scientific  Dialogues  intended  for  the  instruction  and  entertainment  of 

young  people.     12mo.     London,  1852          .  .  .  .  .  .    0  75 

•  -    Dialogues  on  Chemistry.    2  vols.    12mo.        .  .  .  .  .     2  75 

Quelques  points  de  Science  dans  1'Antiquite.     Physique,  Metrique,  Musique. 


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Kane  (Sir  Robert).     Elements  of  Chemistry,  theoretical  and  practical,  including  the 

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Kemp  (T.  L.)     The  Phasis  of  Matter;  being  an  Outline  of  the  Discoveries  and  Applica 

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Knapp,  Ronolds,  and  Kichardson.     Chemistry  in  its  application  to  the  Arts 

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K  y  an  (J.  II.)    On  the  Elements  of  Light,  and  their  identity  with  those  of  Matter,  Radi 

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Laboulaye.     Dictionnaire  des  Arts  et  Manufactures,  de  1'Agriculture,  des  Mines,  etc. 

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plete  .  .  .  .  15  OC 

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vols.)  .  .  .  .  .  .  .  .    5  Ot 

JLacan  (E.)    Esquisses  Photographique1:  a  propos  de  1'Exposition  Universelle  et  de  la 

Guerre  d'Orient.    12mo.    Paris,  1856         .  .  .  .  .  .    0  75 

Lambert.    Sur  la  Meteorologie.    4to.         .  .  .'  .  .  .    0  25 

Lame  (<i.)    Cours  de  Physique  de  1'Ecole  Polytechnique.    2  yols.,  en  3  Parties.    8vo., 

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Lardlier  (D.)    Handbook  of  Natural  Philosophy.    Hydrostatics,  Pneumatics,  and  Heat. 

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A  Treatise  on  Heat.     12mo.    London,  1S56    .  .100 


Lassaigue.     Dictionnaire  des  Reactifs  Chimiques  employes  dans  toutes  le   "xperiences. 

Svo.  tig.    Pnris,  1889      .  .  .  .  .  .  .  .250 

Laurent  (J*  .)    Precis  de  Cristaliographie  suivi  d'une  Methode  Simple  d'Analyse  au  cha- 

lumeau.     12mo.     Paris  .  .  .  ...  .  .     0  37 

Laurent  (Aug.)    Methode  de  Chimie.    Precedee  d'un  Avis  au  Lecteur,  par  M.  Biot,    1 

vol.,  8vo.,  avec  figures  dans  le  texte.     Paris,  1854    .  .  .  .  .200 

Laurent  (A.)    Chemical  Method,  Notation,  Classification  and  Nomenclature.    Trans 
lated  by  Odliag.     London,  1855    .  .  .  ,  .  .  .    3  50 
(Cavendish  Society  Publication.) 

Le  Gray.     Nouveau  Trait e  de  Photographic  sur  papier  et  dur  verre.    Svo.    Paris,  1S51  .    0  T5 

Lehmann.     Physiological  Chemistry.     With  Illustrations.   2  vols.   Svo.    Philadelphia, 

1856,  .  .  .  .  .  •  .  .  .  .    6  00 

Chemical  Physiology.    Translated  by  J.  C.  Morris.     Philadelphia,  1856  .  .    225 

— Precis  de  Chimie  Physiologique  Anirnale.   Traduction  du  Professeur  Drion.    Paris, 

1855.     1  vol.,  gr.  18mo.,  avec  fig.  :....;,  j     .  .  •  ..  .  .  .    1  25 

HL.  Bailliere,  29O  I***oatttcay,  wT.  Y. 


Standard  Scientific  Works. 


L'Heritier  (S.  I>.)     Traite  de  Chimie  Pathologique  ou  Recherches  chimiques  sur  les 
solide*  et  les  liquides  du  corps  humain,  dans  leurs  rapports   avec  la  Physiologic  et  la 
Pathologic.     Svo.     Paris,  1842     .  .  .  .  .  .  .     2  25 

Le  Normand.     L'art  du  distillateur  des  eaux-de-vie.    2  vols.,  Svo.     Paris,  1817  .    300 

Lei  cbours.     A  Treatise  on  Photography,  by  J.  Egerton.     Svo.     London,  1843  .    250 

Lerebours  et  Secretan.    Traite  de  Photographic.    5e  edit.    Svo.  .  .  .    1  00 

Levesque.     Art  of  Brewing  and  Malting.    4th  edit.     Svo.     London,  1847          .  .700 

Liebig  ( J.  V.)    Chemistry  and  Physics,  in  relation  to  Physiology  and  Pathology.    2d  edi 
tion.    Svo.        .  .  .  .  .  .  .  .  .    0  75 

Nouvelles  Lettres  sur  la  chimie,  traduites  par  Charles  Gerhardt.    12mo.    Paris, 

1852  .  .  .  .  .  .  .  .  .  .    0  75 

— — — —    Letters  on  Chemistry.     12mo.     London  .  .  .  .  .     2  00 

Researches  on  the  Chemistry  of  Food.     Svo.     London .  .  .  .     1  62 

Principles  of  Agricultural  Chemistry,  with  special  reference  to  the  late  researches 

made  in  England.     Svo.     London,  1855      .  .  .  .  .  .     1  12 

Handbook  of  Organic  Analysis,  containing  a  detailed  account  of  the  various 

methods  used  in  determining  the  elementary  composition  of  Organic  Substances.    Edited 

by  Hoffman.  Post  Svo.,  woodcuts.  London,  1853 .  .  .'  .  .150 

Liebig  and  Kopp's  Annual  Report  of  the  Progress  of  Chemistry,  <tc.  4  vols.,  cloth. 

1853.     (To  be  continued. )  .  .  .  ...  ^          .  .  .1000 

Light :  It  Nature,  Sources,  Effects,  and  Applications.  Illustrated  by  a  Photograph.  12mo. 

London, 1856    .  .  .  .  .  .  .  .  .    1  25 

Long  (C.  A.)  Practical  Photography  on  Glass  and  Paper.  2d  edit.  12mo.  Sewed.  1856.  031 
Love  (T.)  The  Art  of  Cleaning,  Dyeing,  and  Scouring,  Ac.  12mo.  London,  1S54  .  2  25 
Low  (David;.  Au  Inquiry  into  the  Nature  of  the  Simple  Bodies  of  Chemistry.  3d  edit. 

Svo.    London,  1856         .  .  .  .  .  .  .  .    2  75 

Lowig.     Principles  of  Organic  and  Physiological  Chemistry,  by  D.  Breed.    Svo.    Phila 
delphia,  1853    .  .  .  .  .  .  .  .  .    8  50 

Mackenzie  (C,)  One  Thousand  Processes  in  Manufactures,  and  Experiments  in  Chemis- 

Svo.    London,  1S25.     Half  bd.    .  .  .  .  .  .  .    8  50 

'•  Theory  and  Experiments  in  Chemistry.  Svo.  London,  .  .  .  6  50 

McGauley  (Rev.  J.  AV.)  Lectures  on  Natural  Philosophy.  2  vols.  Svo.  London, 

1S50.     Half  bd.  .  .  .  .  .  .  .  .    5  00 

Malaguti  (F.)  Lecons  de  Chimie  Agricole,  Professees  in  1847.  18mo.  Paris,  1856  .  1  00 
— — ( J.)  Lecons  Elementaires  de  Chimie.  2  vols.  12mo.,  avec  104  figures  intercalees 

dans  le  texte.     Paris,  1853  .  .  .  .  .  .  .    2  50 

Marcet(AV.)  On  the  Composition  of  Food,  and  how  it  is  Adulterated;  with  practical 

directions  for  its  analysis.  Svo.  London,  1856  .  .  .  .  .  2  00 
Marters.  Esquisse  d'une  nouvelle  classification  Chimique  des  Corps.  4to.  .  .  0  25 
— --  Combustion  de  la  vapeur  alcoolique  et  etheree,  autour  d'un  fil  de  Platine.  4to.  .  0  i5 

Sur  la  theorie  Chimique  de  la  Respiration  et  de  la  Chaleur  Animal.    4to.  .    0  50 

Martins  (A.)    Handbuch  der  Photographic.    Dritte  auflage.    Svo.    Wien,  1852  .    2  3: 

Mather  (James).    Coal  Mines,  their  Dangers  and  Means  of  Safety.    Svo.,  woodcuts. 

London, 1853    .  .  .  .  .  .  .  .  .    1  12 

Mattenci.  Cours  Special  sur  1'Induction,  le  Magneti^ne  et  sur  les  relations  entre  la  Force 

Magnetique  et  les  Actions  Moleculaires.  Svo.  Paris,  1854  .  .  .  .  1  50 

Mattcucci  et  Savi.  Traite  des  phenomenes  Electro-Physiologiques  des  animaux. 

Svo.    Paris,  1S41  .  .  .  .  .  .  .  .    2  00 

Matthews  (AV.)     Compendium  cf  Gas  Lighting.    12mo.    London     .  .  .    125- 

Historical  Sketch  and  Origin  of  Gas  Lighting.    12mo.     London  .  .    2  25 

Memoares  d' Agriculture,  d'Economie  Rurale  et  Domestique,  publics  et  par  la  Societe  Im- 

periale  et  Centrale  d'Agriculture.     Annee  1S54.     lere  partie,  Svo.     Paris,  1855  .     1  50 

Messier.     Observations  sur  les  grandes  Chaleurs,  la  Secheresse,  etc.,  de  la  Seine  a  Paris, 

4to.     Pendant  1793          .  .  .  .  .  .  .  .    0  50 

Metcalie  (S.  T  )    Caloric  ;  its  Mechanical,  Chymical,  and  Vital  Agencies  in  *he  Pheno 
mena  of  Nature.     2  vols.,  Svo.      .  .  .  .  .  :    .  '  .  10  50 

Mialhe.     Chimie  appliquee  a  la  Physiologic  et  a  la  Therapeutique.    Svo.    Paris,  1S55      .    2  5(/ 

Miller  (AV.  A.)    Elements  of  Chemistry,  Theoretical  and  Practical,  extensively  illus 
trated.    3  vols.    8vo.    London,  1855-57    .  .  .  .  .  14  00 
Just  Completed. 

Millar    (James).     Elements  of  Chemistry.    Svo.    London  .  .  .    8  75 

Miller  (AV.)    (Cashier  to  the  Bunk  of  England.)    Decimal  Tables  used  at  the  Bank  of 

England,  for  reducing  Gross  weight  of  Gold  and  Silver  to  Standard.    4to.    London,  1854    1  25 

Milfoil  (M.  E.)    Etudes  de  Chimie  Organique  faites  en  vue  des  Applications  Physiolo- 

logiquos  et  Mcdicales.     Svo.     Lille,  1S4S)     .  .  »  .'  .  .  .     0  75 

II.  JSaitliere^ 


10  Standard  Scientific  Works. 

Ifliilon  (iTT.  E.)    Des  Phenomenes  qui  se  produisent  du  contact  de  PEau  et  du  Ble  et  de 

leur  Consequences,  Industrielles.    8vo.    Paris,  1854         ;,»  .  .  .050 

Mitchell  (T.)  Manual  of  Practical  Assaying,  intended  for  the  use  of  Metallurgists, 
Captains  of  Mines,  and  Ascayers  in  general.  With  a  copious  table,  for  the  purpose  of 
ascertaining  in  Assays  of  Gold  and  Silver  the  precise  amount,  in  ounces,  pennyweights, 
and  grains,  of  noble  metal  contained  in  one  ton  of  ore,  from  a  given  quantity.  1  vol., 
8vo.  2nd  edit.  London,  1854  .  .  .  .  .  .  5  00 


Treatise  on  the  Adulterations  of  Food,  and  the  Chemical  means  employed  to 


detect  them.     Containing  Water,  Flour,  Bread,  Milk,  Cream,  Beer,  Cider,  Wines,  Spirit 

uous  Liquors,  Coffee,  Tea,  Chocolate,  Sugar,  Honey,  Lozenges,  Cheese,  Vinegar,  Pickles, 

Anchovy  Sauce  and  Pasta,  Catsup,  Olive  (Salad)  Oil,  Pepper,  Mustard.    12mo.    Lon 

don,  184S          .  .  .  .  .  .  .  .  .    1  50 

Moisj  ii«.     Traite  de  Telegraphic  Electrique.    8vo.,  and  atlas.    Paris,  1852         .  .    3  75 

--    Repertoire  d'Optique.    4  vols.,  8vo.    Paris,  1849-50.    (Very  scarce.)      .  . 

Morehead  (v  .)    Essay  on  Inebriating  Liquors  and  Distillation.    8vo.    London  .    475 

ITIorfit  (C.)    A  Treatise  on  Chemistry  applied  to  the  Manufacture  of  Soap  and  Candles. 

New  edition.     8vo.,  woodcuts.     Philadelphia,  1S56  .  .  .  .     6  00 

Mulder  (G.   J.)     The   Chemistry   of  Vegetable   and   Animal    Physiology,   with   intro 

duction  and  notes  by  J.  E.  W.  Johnston,  and  twenty  illustrations,  colored  and  plain. 

8vo.,  cloth        ;  .  .  .  .  .  .  .  .     8  50 

Muller.     Principles  of  Physics  and  Meteorology.    Illustrated  with  500  Woodcuts,  and  2 

colored  plates.     Svo.     London,  1847  .  .  .  .  .  .    4  GO 

Murpliy  (Rev.  R.)    Elementary  Principles  of  the  Theories  of  Electricity,  Heat,  and 

Molecular  Actions.     Part  I.     Svo.     Cambridge  (England),  1832        .  .  .    2  25 

Murpliy  (P.)    Rudiments  of  the  primary  forces  of  Gravity,  Magnetism,  and  Electricity 

in  their  Agency  on  the  Heavenly  Bodies.     Svo.     London,  1880  .  .  .    4  00 

Murray.    System  of  Chemistry,    4  vols.,  Svo.    London          .  .  .  .  15  75 

Sketch  of  Chemistry.    12mo.    London  .  .  .  .  .    2  25 

Manual  of  Chemical  Experiments.    12mo.    London    .  .  .  .    1  50 

Chemical  Tables  and  Diagrams.    Svo.    London  .  .  .  .    1  00 

•  --    Elements  of  Chemistry.    4  vols.,  Svo.    London  .  .  .  .    7  50 

Muspratt  (Dr.  S.)     The  Use  of  the  Blowpipe,   in  the  Qualitative  and  Quantitative 

Examination  of  Minerals,  Ores,  Furnace  products,  and  other  metallic  combinations. 

By  Plainer.     8vo.,  cloth  .  .  .  .  .  .  .    3  00 


Chemistry  Theoretical,  Practical,  and  Analytical,  as  applied  and  relating  to  the 


Arts  and  Manufactures.     Royal  Svo.     Div.  1  and  2.     London,  1856.     Each      .  .     2  C2 

Each  division  of  this  fine  work  contains  4  portraits  (engraved  on  steel)  of  the  most 

celebrated  chemists. 

Will  be  completed  in  about  C  divisions. 
Napier  ( J.)    Manual  of  Electro-Metallurgy.    Post  Svo.    1858  .  .  .    1  00 

A  Manual  of  the  Art  of  Dyeing.    Svo,  with  illustrations.    London,  1853  .    2  25 

Nesbit  (J,  C.)    On  Agricultural  Chemistry,  and  the  Nature  and  Properties  of  Peruvian 

Guano.    3d  edition.    Svo.    London,  1S56  .  .  .  .  .    1  25 

Nisbet  (W.)    Dictionary  of  Chemistry.    12mo.    London        .  .  .  .    2  50 

Nicollet  (H.)    Atlas  de  Physique  et  de  Meteorologie  Agricoles.    Grand  in-fol.,  de  18  pi. 

col.,  avec  tableaux  et  texte.    Paris,  1855  .  .  .  .  .  .  18  50 

Noad  (H.  M.)  A  Manual  of  Electricity,  including  Galvanism,  Magnetism,  Diamagne- 
tism,  Electro-Dynamics,  Magneto-Electricity,  and  the  Electric-Telegraph.  4th  edition, 
entirely  rewritten.  Part  I.  Electricity  and  Galvanism.  Svo.  London,  1856  .  5  00 

« Chemical  Manipulation  and  Analysis  Qualitative  and  Quantitative.  With  an  intro 
duction  explanatory  of  the  general  principles  of  Chemical  Nomenclature,  Ac.  8vo. 
London, 1S52  .  .  .  .  .  .  .  .  .  8  00 

Lectures  on  Chemistry.    Svo.    London         .  .  .  .  .    3  75 

Normandy.    Commercial  Handbook  of  Chemical  Analysis.    Post  Svo.    London,  1850  .    8  75 

A  Practical  Treatise  on  Chemical  Analysis,  Quantitative  and  Qualitative.    By 

Rose.    2  vols.,  Svo.    London,  1848  .  .  .  .  .  .  10  25 

•    An  Introduction  to  ditto,    Svo.    London       .  .  .  . 

Orfila  (M.  P.)    Elements  of  Modern  Chemistry.    Svo.    London 
Ottley(W»C.)    Dictionary  of  Chemistry  and  Mineralogy.     Svo.    London      . 
Paris  (J.  A.)    Elements  of  Medical  Chemistry.    Svo.    London 
Parnell.    Treatise  on  Dyeing  and  Calico  Printing.    Svo.     London 


Elements  of  Chemical  Analysis,  Qualitative  and  Quantitative.    Svo.    London.  1S45. 


Reduced  to      .  •  '-.  ••-  .  .  .  .  .  .  .     2  75 

Applied  Chemistry  in  Manufactures.     Vols.  1  and  2.     Svo.    London.    Each         .    8  75 

Payen.  Cours  de  Chimie  Appliquee,  professe  a  1'Ecole  Centrale  des  Arts  et  Manufactures, 
et  au  Conservatoire  des  Arts  et  Metiers.  Redige  par  Dellisse  et  Poinsot.  Ire  partie  : 
Chimie  Organique.  Svo.,  avec  atlas  folio  de  50  planches.  Paris,  1847  .  .  9  00 

W.  Ballliere,  29O  Broadway,  JIT.  I". 


Standard  Scientific  Works.  11 


Payen.  Precis  dc  Chimie  Industrielle,  a  1'usag^  des  Ecoles  preparatoires  aux  Profes 
sions  Industrielles  des  fabricants,  et  des  agriculteurs.  3d  edit.  8vo.,  avec  atlas  de 
planches  in  8vo.  Paris,  1855  .  .  .  *  .  .  .  4  50 

Payen  et  Richard.  Precis  d'Agriculture  theorique  et  pratique.  2  vols.,  8vo. 

Paris,  1861.  .  .  .  .  •  •  •  .  .  8  75 

Peckston  (T,  S.)    Treatise  on  the  Manufacture  of  Gas.    Svo.    London         .  .    7  75 

Peclet  (E.)    Traite  elementaire  de  Physique.  4rae  edition.  2  vols.,  8vo.,  atlas,  Paria,  1847    3  75 

Traite  de  la  Chaleur,  consideree  dans  ses  applications.    Troisieme  edition  entiere- 

rnent  refondue.     Un  atlas  de  122  planches  et  uu  vol.  de  texte.    Liege  .  .  12  50 

Do.,  2  vols.,  4to.,  et  atlas.     Paris  .  .  .  .  .  .  17  50 

Le  supplement  separement,  1853.    4to.  .  .  .  .  .    2  25 

Pelouze.     Traite  de  1'Eclairage  au  Gaz  tire  de  la  Houille,  des  Huiles,  de  Resines,  etc. 

1  vol.,  8vo.,  et  24  pi.    (Scarce.)    ....... 

Pclouz  et  Fremy.     Traite  de  Chimie  generate,  comprenant  les  applications  de  cette 

Science  a  1'Analyse  Chimique,  a  1'Industrie,  a  1'Agriculture,  et  a  1'llistoire  Naturello. 
2nde  edit.    Tomes  1  a  5  et  atlas.    Paris,  1854-36      .  .  .  .  .  12  00 

II  y  aura  un  6e  vol.,  qui  sera  donne  gratis. 

Abrege  de  Chimie.    Troisieme  edition,  conforme  aux  nouveax  programmes  de 

1'enseignement  scientifique  des  Lycees.    8  vol.,  grand  18mo.,  avec  174  figures  intercalees 
dans  le  texte.    Paris,  1855  ....... 

Notions  Generates  de  Chimie.     Un  beau  volume  imprime  avec  luxe,  accompagne 

d'un  Atlas  de  24  planches  en  couleur,  cartonne.    Paris,  1853  .  .  .    5  60 

Peltier     (A,)     Meteorologie.      Observations    et     Recherches    experimentales.      Svo. 

Paris,  1840       .  ...  .  .  .  .  .  .    2  00 

Pereira.    Lectures  on  Polarized  Light.    Second  edition,  greatly  enlarged  from  materials 

left  by  the  author.    Edited  by  Prof.  Powels,  of  Oxford.    12mo.,  woodcuts.    London,  1854    225 

Persoz.  Traite  theorique  et  pratique  de  1'impression  des  tissus.  4  beaux  vol.,  Svo.,  avec 
165  figures  et  429  echantillons  d'etoffes,  intercales  dans  le  texte,  et  accompagnes  d'un 
atlas  de  10  pi.  4to.,  gravees  en  taille-douce,  dont  4  sont  coloriees.  Ouvrage  auquel  la 
societe  d'encouragement  a  accorde  une  medaille  de  3,000  fr.  Paris,  1846  .  .  17  00 

Pharmaceutical  Journal  and  Transactions.  Yols.  1  to  15.    Half  bound.  London, 

1841  to  1S56      .  .  .  .  .  .  .  .  .  50  00 

Annual  Subscription  (published  monthly)  .  .  .  .    8  75 

Pharmacopoeia.  The  New  London,  including  also  the  Dublin  and  Edinburgh  Phar 
macopoeias  by  J.  B.  Nevins,  M.D.  Svo.  London,  1851.  .  .  t  .  .  6  00 

Phillips  (.1.  A.)  Gold  Mining  and  Assaying;  a  Scientific  Guide  for  Australian  Emi 
grants.  12uio.  With  woodcuts,  London,  1852.  .  .  .  .  .  1  00 

Manual  of  Metallurgy.     Post  Svo.    New  edit.    London,  1854.    .          ...  .    875 

Phillips  (R.)    A  Million  of  Facts  of  correct  data  and  elementary  constants  in  the 

entire  circle  of  the  Sciences,  and  on  all  subjects  of  speculation  and  practice.    New  edit. 
12mo.    1856.     .  .  .  .  .  .  .  .  .    8  62 

Philosophical  Transactions  of  the  Royal  Society  of  London,  from  1S25  to  1851, 

inclusive,  forming  25  vols.  4to.    Half  bound  in  Russia  ...  180  00 

(Published  price,  £70  unbound.) 

Picsse  (S.)  The  Art  of  Perfumery,  and  the  Method  of  obtaining  Odors  of  Plants  ; 
with  instructions  for  the  Manufacture  of  Perfumes  for  the  Handkerchief,  Scented  Pow 
ders,  Odorous  Vinegars,  Dentifrices,  Pomatums,  Cosmetiques,  Perfumed  Soap,  Ac. 
With  appendix,  Ac.  Crown  8vo.,  cloth.  London,  1856.  .  .  .  .  2  25 

Plattner  (C.  F.)  Tableau  de  Caracteres  que  presentent  au  Chalumeau  les  alcalis,  les 
terres  et  les  oxydes  metalliques,  soil  seuls,  soil  avec  les  reactifs.  Traduit  de  1'Allemand 
par  Sobrero.  4to.  Paris,  1843  .  .  .  .  .  .  .  0  60 

The  Use  of  the  Blowpipe  in  the  Qualitative  and  Quantitative  Examination  of 

Minerals,  Ores,  furnace  products,  &c.    Svo.    London,  1850  .  •  .    8  CO 

Poisson  (S.  D.)    Theorie  Mathematique  de  la  chaleur.    Svo.    1S35  .  .050 

Poll il let.      Elements  de  Physique  Experimentale  et  de  meteorologie.     7me  edition. 

2  volumes,  Svo.  de  texte  et  uu  volume  de  40  pi.  8vo.,  4to.     Paris,  1856  .  .    4  50 
Prechtl  ( J.  J.)    Technologische  Encyclopaedic  oder  alphabetisches  handbuch  der  Tech 
nologic  der  Technischen  Chemie  und  des  Maschirienwesens.    Vols.  1  to  18.    Svo.,  und 
plates  fol.         ......... 

Prideaux  (T.  S.)    On  Economy  of  Fuel,  particularly  with  reference  to  Reverberatory 

Furnaces  for  the  Manufacture  of  Iron,  and  to  Steam  Boilers.    12mo.t  cloth   .  .080 

Prout  (W.)    Treatise  on  Chemistry,  Meteorology,  etc.    Svo.  London  .  .    4  50 

QueteIet(A.)    Positions  de  Physique.    8  vols.  ISmo.    Brussels,  1S34  .  -200 

Hammelsberg*  (C.  F.)    Lehrbuch  der  Stochiometrie  und  der  Allgemeinen  theoreti- 

schen  chemie.    Svo.    Berlin,  1S42  .  .  .  .  .  .    1  75 

-  Anfangsgrunde  der  quantitativen  Mineralogisch,  und  Metallargisch,  anaytischen 
Chemie  durch  Beispiele  erlautert.    Svo.    Berlin,  1845  .  .  .  .    1  75 

— —    Leisfaden  fur  die  Qualitative  Chemische  Analyse,  mit  besonderer  Rucksicht  auf 

H.  Rose,  Handb.  der  analyt.  Chemie.    Svo.    Berlin,  1843      .  .  .  .    0  75 


Iff.  Baillicre,  29O  Broadway, 


12  Standard  Scientific  Works. 

Itasptlil  (F.  V»)  Nouveau  Systemc  de  Chimie  Organique,  fonde  sur  de  nouvellcs 
methodes  d'observations,  precede  d'un  Traite  complet  sur  1'art  d'observer,  de  manipuler 
en  grand  et  en  petit,  dans  le  laboratoire  et  sur  le  porte-objet  du  microscope.  Deuxieme 
edition,  entierernent  refondue,  accompagnee  d'un  atlas  in-4  de  20  planches  de  figures 
dessinees  d'apres  nature,  gravces  et  coloriees  avec  le  plus  grand  soin.  3  vols.,  Svo.,  atlas 
4to.  Paris,  1838  .  .  .  .  .  .  .  .  7  5C 

Nouveau  Systeine  de  Physiologie  vegetale  et  de  Botanique,  fonde  sur  les  methodes 

d'observations  developpes  dans  le  uouveau  systeme  de  chimie  organique,  accompagne 
de  60  planches  contenant  pres  de  1,000  figures  d'analyse  dessinees  d'apres  nature  et 
gravees  avec  le  plus  grand  soin.  2  forts  vol.,  8vo.,  et  atlas  de  60  planches.  Paris, 
1837  .  .  .  .  .  .  .  .  .  7  5(1 

^— • —    Le  meme  ouvrage,  planches  coloriees  .  .  .  .  .  12  50 

Reccti.  Theorie  Generate  sur  les  Effets  Dynamiques  de  la  Chaleur.  4to.,  avec  planche. 

1S54  .  .  .  .  .  .  .  .  .  3  00 

Sicilian  It  (It,  II.)  Cours  Elementaire  de  Chimie,  a  1'usage  des  Facultes,  des  Etablis- 
sements  d'Enseignement  secondaire,  des  Ecoles  Normales  et  des  Ecoles  Industrielles.  4 
vols.  12mo.  4th  edit.  Paris,  1853-4  .  .  .  .  .  .  5  00 

Elements  of  Chemistry.     Translated  by  Betton   and  Taber.     2  vols.    Svo.     700 

woodcuts.     Philadelphia,  1853      .  ...  .    7  50 

Relations  des  Experiences  entreprises  pour  determiner  les  principales  lois  et  les 

donnees  numeriques  qui  entrent  dans  le  calcul  des  Machines  a  Vapeur.    4to.     Paris, 
1847.    (Scarce.)  .  .  .  .  .  .  .  .  10  00 

Cours  Elementaire  de  Physique.   4  vols.,  18mo.,  anglais,  avec  figures  dans  le  texte. 

Sous  presse       ......  '  -.  . 

An  Elementary  Treatise  on  Crystallography.    Illustrated  with  108  Wood  Engrav 
ings,  printed  on  black  ground.    Svo.    London,  1848  .  .  .  .    0  75 

Premiers  Elements  de  Chimie.    1  vol.,  18mo.,  avec  figures  dans  le  texte.    Paris, 


1850  .  .  .  .  .  .  .  .  .  .    1  25 

Reichenbach  (Baron  Charles.)    Physico-Physiological  Researches  on  the  Dyna 
mics  of  Magnetism,  Electricity,  Heat,  Light,  Crystallisation,  and  Chemism,  in  their  Rela 
tions  to  Vital  Force.   The  complete  work,  from  the  German  second  edition,  with  additions, 
a  preface,  and  critical  notes,  by  John  Ashburner,  M.D.    Svo.    With  woodcuts  and  one 
plate.     London,  1850      .  .  .  .  .  .  .  .    3  00 

Reid  (D.  B.)    Illustrations  of  the  Theory  and  Practice  of  Ventilation,  with  remarks  on 

Warming,  Exclusive  Lighting,  and  the  Communication  of  Sound.    Svo.     London,  1844  .    4  80 
..     ...  .          Rudiments  of  Chemistry,  with  illustrations  of  the  Chemistry  of  Daily  Life.    4th 

edit.    12mo.    London,  1851          .  .  .  .  .  .  .    0  75 

Repertoire  de  Pharmac:e.    6  vols.    Svo.    1846-1850  .  .750 

Richardson  (C.  JT.)    Popular  Treatise  on  the  Warming  and  Ventilation  of  Buildings. 

18  plates.     8vo.,  hi.  cf.    London,  1831       .  .  .  .  .  .    2  00 

Rintoul  (A.  N.)    A  Guide  to  Painting  Photographic  Portraits,  Draperies,  Background, 

etc.,  in  Water  Color.    With  colored  diagrams.     12mo.    1S55  .  .  .    0  50 

Roberts  (W.  L.)     Scottish  Ale  Brewer  and  Maltster.    Svo.    London  .  .500 

Robertson  (H.)    A  General  View  of  the  Natural  History  of  the  Atmosphere,  &c.    2 

vols.,  Svo.,  cf.    Edinburgh,  1808  .  .  .  .  .  .    2  00 

Rove  (If.)  Traite  pratique  d'analyse  chimique,  suivi  de  tables  servant  dans  les  analyses 
a  calculer  la  quantite  d'une  substance  d'apres  celle  qui  a  ete  trouvee  dans  uue  autre 
substance ;  traduit  de  1'allemand  sur  la  quatrieme  edition  par  A.  J.  L.  Jourdan.  Nou- 
velle  edition,  avec  des  notes  et  additions,  par  M.  Peligot,  professeur  de  chimie  au  Con 
servatoire  des  arts  et  metiers.  2  vols.,  Svo.,  fig.  Paris,  1843 

Practical  Treatise  on  Chemical  Analysis,  including  Tables  for  calculations  in  Ana 
lysis.     With  notes  and  additions  by  A.  Normandy.     2  vols.,  Svo.,  cloth.     London  .  10  25 

Analytical  Manual  of  Chemistry,  by  Griffin.    Svo.    London      .  .  .    4  75 

Ausfuhrliches  Handbuch  der  Analytisches  Chemie.    2  vols.,  8vo.,  hf.  bound  calf. 

Braunschweig,  1851         .  .  .  •  •  •  •  .    8  00 

Roseleur  (.4.)  Manipulations  Hydroplastiques.  Guide  pratique  du  doreur,  de  1'argen- 
teur  et  du  galvanoplastie  (avec  90  figures  en  galvanoplastie  intercalees  dans  le  texte). 
Svo.  Paris,  1856  .  .  .  .  •  •  •  .  3  75 

Runge  (F.  F.)    Chemistry  of  Dyeing.    Part  1.    Svo.    London          .  .  .    1  50 

Kyland  (A»)  Treatise  on  Assay  of  Gold  and  Silver  Wares.  Post  Svo.  London,  1S52  .  175 
Sabine  (E.)  Magnetical  Observations  at  Hobarton.  Vol.  2,  royal  4to.  London,  1S52  .  12  00 
Sacc  (F.)  Precis  Elementaire  de  Chimie  Agricole.  2e  edit.  12mo.  Paris,  1855  .  1  00 

Safety  Lamps  for  Miners,  etc.  Knapp's  Chemical  Technology.  Vol.1.  1856  900 
Sanders  (Or.  J.  TI.)  Practical  Manual  on  the  Use  of  the  Blowpipe  «»•  •  . 

Will  be  published  in  January,  1857. 

Santini.    Teorica  degli  objettivi  acromatici.    4to     .  .  .  .  .050 

Scheerer  (T.)  An  Introduction  to  the  Use  of  the  Blowpipe  ;  together  with  a  descrip 
tion  of  the  Blowpipe,  characters  of  the  important  minerals.  Translated  by  II.  L.  Blan- 
chard.  12mo.  London,  1856  .  .  .  .  .  •  .  1  00 

J9T.  Xtailliere,  29O  Broadway,  *ft\  I*. 


Standard  Scientific  Works.  13 

Sclioedlcr  and  Uledlock.  The  Book  of  Nature  ;  an  elementary  introduction  to  the 

Sciences  of  Physics,  Astronomy,  Chemistry,  Ac.,  &c.  8vo.  London,  1861  .  .  3  50 

Sell  rode  r  (H.)  Die  Molecular  volume  der  Chemischen  Verbindungen  im  festen  und  flus- 

sigen  Zustande.  8vo.  Mannheim,  1843  .  V^'  .  .  .  .100 

Scoffern.  Chemistry  of  the  Imponderable  Agents;  including  the  Principles  of  Light, 

Heat,  Electricity,  and  Magnetism.  8vo.  London,  1855  .  .  .  .  1  00 

Manufacture  of  Sugar  in  the  Colonies.    8vo.     London  .  .  .325 

Elementary  Chemistry  of  the  Imponderable  Agents  and  of  Inorganic  Bodies.    8vo. 

London, 1855   .  .  .  .  .  .  .  .  .    1  50 

Chemistry  no  Mystery.    12mo.    London        .  .  .  .  .    1  50 


Ncoresby  (%%r.)    Magnetical  Investigations.    3  vols.,  8vo.    London,  1852         .  .300 

Slieir  (John).    Directions  for  Testing  Cane-Juice.    12mo.,  cloth       .  .  .087 

IS  ill  i  c  (A.)    Instinct  arid  Reason;  deduced  from  Electro-Biology.     8vo.,  cloth  .  .    5  00 

-  Elements  of  Electro-Metallurgy.    Illustrated  with  woodcuts.    8vo.,  cloth  .    1  50 
Sm  ;tli  (It.  SE.)    Italian  Irrigation  ;  being  a  Report  of  the  Agricultural  Canals  of  Pied 

mont  and  Loutbardy  ;  addressed  to  the  Directors  of  the  East  India  Company.    2  vols. 

8vo  ,  and  plates,  folio,  cloth.    Edinburgh,  1855        .  .  .  .  .    9  00 

Smith  (IS.)    Practical  Dyer's  Guide.     8vo.    London  .  .  .  .1900 

--    Dyers'  Instructor.    12mo.>  London  .  .  .  .  .  .    6  50 

Solly  (E.)  Introduction  to  Rural  Chemistry.  Svo.  London  .  .  .150 

-  Syllabus  of  Lectures  on  Chemistry.     Svo.    London     .  .  .  .    1  DO 
Suulxiran.     Traite  de  Pharmacia  theorique  et  pratique.    8e  edition.    2  forts  vol.    Svo., 

uvec  t>3  fig.  imprimees  dans  le  texte.     Paris,  1847    .  .  .  .  .    4  00 

-  Precis  elementaire  de   Physique.    2e  edit.,   augmentee.    1  vol.,  Svo.,   avec    18 
planches  4to.     Paris,  1844  .  .  .  .  .  .     1  25 

Sutton  (  I'.)    The  Calotype  Process:  a  Handbook  of  Photography  on  Paper.    Svo.    Lon 

don,  1&55          .  .......        75 


Principles  of  Chemistry.    Svo.     London      .  .  .  .360 

Table*  generates  des  Comptes  Rendus  des  seances  de  1'  Academic  des  Sciences,  publiees  par 
MM.  les  secretaires  perpetuels,  conformement  a  une  decision  de  1'Academie,  en  date  du 
13  juillet  1835.     Tomes  1  a  31.  3  aout  1835  a  30  decembre  1850.    4to.    Pari?,  1854  .    6  00 

Tardieu  (A.)    Voiries  et  cimetieres.    Svo.    Paris,  1S52        .  .  .  .100 

T  ate  (T.)    The  Little  Philosopher  ;  or,  the  Science  of  Familiar  Things  ;  in  which  the  Prin 
ciples  of  Nature  and  Experimental  Philosophy  are  Systematically  Developed  from  the 
Properties  and  Uses  of  Familiar  Tilings.    Vol.1.    ISmo.    London,  1855  .  .     1  12 

-  (C.)     Theory  and  Experiments  in  Chemistry.    Svo.    London    .  .  .    6  50 

1  lienard.    Traite  de  Chimie  elementaire.    6e  edit.    5  vols.    Paris,  1834-6 

Very  scarce. 
'S  lii«-me  (F.  W.)    Die  Physik  in  ihre  Beziehung  zur  Chemie,  Oder  diejenizen  lehren  der 

Physik,  &c.     Svo.     Leipzig,  1840  .  .  .  .  .  .75 

Thomson  (T.)    Practical  Dyer's  Assistant.    12mo.    London  .  .     1  5D 


Chemistry  of  Organic  Bodies— Vegetables.    1  large  vol.,  Svo.,  pp.  1092,  boards. 


London,  1838  .  .  .  .  .  .  .  .  .600 

-  Heat  and  Electricity.    2d  edition.    1  vol.,  Svo.    Illustrated  with  woodcuts    Lon 

don,  1S39          .  .  .    4  O'J 

--    Chemistry  of  Animal  Bodies.    Svo.,  cloth      .....    4  <;» 

-  History  of  Chemistry.    2  vols.    12mo.    Scarce  .  .  .  .    2  5>l 

-  Treatise  on  Brewing  and  Distillation.    Svo.    London  .  .  .     1  8.1 

-  Elements  of  Chemistry.    Svo.    London          .  .  .  .'  .8  '2."> 

-  First  Principles  of  Chemistry.     2  vols.,  Svo.    London  .  .  .    9  •  0 

-  Outlines  of  Mineralogy,  Geology,  &c.     3  vols.,  Svo.     .  .  .  .     t)  r,o 

-  System  of  Inorganic  Chemistry.    2  vols.,  Svo.    London  .  .  .12  M 

-  System  of  Chemistry.    4  vols.,  Svo.    London  .  .  .  .  IS  IX) 
Thomson  (K.  D.)    Cyclopaedia  of  Chemistry,  Practical  and  Theoretical,  including 

the  Application  of  the  Science  to  the  Arts,  Mineralogy,  and  Physiology.  8vu  with 
illustrations.  London,  1854  .  .  .  .  .  .  '  .  8  75 

Th  »i  itlh\v»ite  (IV.  H.)  A  Guide  to  Photography  :  Simple  and  Concise  Directions 

for  obtaining  Views,  Portraits,  &c.  9th  edit.  12mo.  London,  1856  .  .  .30 

Tiz-ird  (W.  I,.)    Theory  and  Practice  of  Brewing.    2nd  edit.    Svo.    London,  1846      .     750 

-  brewer's  Journal.     London,  1854     .  .  .  .  .  .     8  25 


et  «a.»dissal.     Dictionnaire  Technologique.    Francais-Anglais-Alle 
inand.     3  vols.,  12.no.     Paris  18»  .  .  . 


T«»: 


<  •liiiswtB  (('.)  Cyclopaedia  of  Useful  Arts,  Mechanical  and  Chemical,  Manufactur 
ng,  Mining  and  Engineering.  2  vols.,  8vo.,  with  splendid  steel  plates  and  woodcuts 
London,  lSf4  .  10 

•  •  •  •  .    I- 

II.  BaiUiere,  99O  Broadway,  J*\  K. 


14  Standard  Scientific  Works. 


Trosseau  et  Rcvcil.    Traite  de  1'art  de  formuler,  comprenant  des  notions  de  Phar- 

macie.    12mo.    1861.    .  .  .  .  .  .  .  .    1  25 

Turner  (E.)    Elements  of  Chemistry,  including  the  actual  State  and  prevalent  Doctrines 

of  the  Science.    8th  edit.    Edited  by  Baron  Liebig  and  Dr.  Gregory.    8vo.  cloth  .    9  00 

Ure  (A.)  A  Dictionary  of  Arts,  Manufactures,  and  Mines,  containing  a  clear  Exposition 
of  their  Principles  and  Practice.  4th  edit.,  corrected  and  greatly  enlarged.  2  vols.,  8vo., 
pp.  8,078,  and  1,600  engravings  on  wood,  cloth.  London,  1858  .  .  .550 

Dictionary  of  Chemistry.    Svo.    London       .  .  .  .  .    6  50 

Van  IVIoiis.     Sur  les  combinaisons  faites  par  le  Pyrophore.    4to.        .  .  .60 

Violette  et  Arcltambaiilt.    Dictionuaire  des  Analyses  chimiques  ou  Repertoire 
alphabetique  des  Analyses  de  tous  corps  naturels  et  artificiels  depuis  la  fondation  de 
la  chimie,  avec  1'indication  des  noms  des  auteurs  et  des  recueils  ou  elles  ont  ete  inserees. 
2  vols.,  8vo.,  a  2  col.    Paris,  1851  .  .  .  .  .    4  00 

Or  half  calf  .  .  .  .  .  .  .  .  .    5  00 

Wallter  ( W.)    The  Magnetism  of  Ships  and  the  Mariner's  Compass  :  being  a  Rudimen 
tary  Exposition  of  the  Induced  Magnetism  of  Iron  in  Sea-going  Vessels.    12mo.    Lon 
don,  1853          .  ......    1  50 

1  (C.  V.)  et  Fail.    Manipulations  Electrotypiques,  ou  Traite  de  Galvanoplas- 

tie,  contenant  la  Description  des  Precedes  les  plus  Faciles  pour  Dorer,  Argenter,  Graver 
sur  Cuivre  et  sur  Acier,  reproduire  les  Medailles  et  les  Epreuves  Daguerriennes,  Metal- 
liser  les  Statuettes  de  Platre,  etc.,  au  moyen  du  Galvanisme.    4me  edition,  18mo. 
Paris,  1855        .........        50 

Watson  (R.)    Chemical  Essays.    5  vols.,  18mo.    London,  1800          .  .  .    2  50 

"Webster  (J.)    Elements  of  Mechanical  and  Chemical  Philosophy.    Svo.  .  .    8  CO 

Weekes  (W.  If.)    A  Memoir  on  the  Universal  Portable  Eudiometer,  an  Apparatus 

designed  for  researches  of  Philosophical  Chemistry.    4to.,  with  plate.    Sandwich,  1838  .    1  00 
Weldon  (W.)    Elements  and  Laws  of  Chemistry.    8vo.    London      .  .  .875 

Wertheim.    Theses  presentees  a  la  Faculte  des  sciences  de  Paris  pour  obtenir  le  grade 
de  docteur  des  sciences  physiques.     Paris  1853         ..... 

Theses  dc  physique,  de  chimie  et  de  mineralogie. 

Will   ct  JLiebigr.     Manuel   Complet  de   Chimie   Analytique,   contenant  des  Notions 
sur  les  Manipulations  Cliimiques,  les  Elements  d' Analyse  Inorganique  Qualitative  et 
Quantitative,  et  des  Principes  de  Chimie  Organique.     2  vols.     18mo    .  .  .    1  25 

Williams  (C.  W.)    Treatise  on  the  Combustion  of  Coal.    4to.    London        .  .    825 

Witts  ti'in.     Practical  Pharmaceutical  Chemistry,  translated  by  S.  Darley.    London,  1858    188 
WoliHer  (F.)    Handbook  of  Inorganic  Analysis.    Translated  and  edited  by  Hofmann. 

12mo.    London  .  .  .  .  .  .  .  .    2  00 

"Wolff  (E.   T,)     Quellen-Litteratur  der    theoretisch-organischen  Chemie,   Ac.    Svo. 

Halle,  1845      .  .  .  .  .  .  .  .  .    1  00 

Woodward  (C.)    A  Familiar  Introduction  to  the  Study  of  Polarized  Light.    2nd  edit. 

Svo.    London,  1851        .  .  .  .  .  .  .  .    1  00 


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XJXTID 


Alchemy.    Figuier,  5. 

Apparatus.   An  Explanatory  Dictionary,  1 

Arts  and  Manufactures.    Ac-ken,  1 . 

Brande,  2 ;  Dodd,4  ;  Exhibition  Lectures,  5  ; 
Knight,  8;  Laboulaye,  8;  Mackenzie,  9; 
Muspratt,  10 ;  Tomlinson,  13 ;  Ure,  14. 

Assaying.  Berthier,  2;  Mitchell,  10;  Phil 
lips,  11 ;  Ryland,  12. 

Blowpipe.  Berzelius,  2;  Griffin,  6;  Mus 
pratt,  10 ;  Plattner,  11 ;  SANDERS,  12 ;  Sheerer, 
12. 

Brewing*.  Accum,!;  Black,  2;  Lacambre, 
8 ;  Levesque,  9  ;  Roberts,  12 ;  Thomson,  13 ; 
Tizzard,  13. 

Caoutchouc.    Manuel-Roret,  3. 

Chemistry.  Brande,  2 ;  Cavendish  Society, 
8;  Chevallier  (Dictionary),  3;  Cuvier,  4; 
Dalton  (Life),  4  ;  Dumas  (Statique),  5 ;  Gal 
loway  (Diagram),  5 ;  Griffith  (Recreation), 
6;  Henry,  7 ;  G.  8.  Hilaire,  7 ;  Johnston,  7 ; 
Joyce,  8 ;  Laurent,  8 ;  Lehmann,  8 .  L'Heri- 
tier,  9 ;  Liebig,  9  ;  Low,  9  ;  Mackenzie,  9 ; 
Martens,  9;  Messier,  9;  Mulder,  10  ;  Mur 
ray,  10 ;  Orflla,  10 ;  Paris,  10  ;  Pelouze  and 
Fremy,  11 ;  Prout,  11 ;  Rammelsberg,  11 ; 
Reid,  12 ;  Schoedler  &  Medlock,  18 ;  Scoffern, 
12;  Smee,  13;  Swedenborg,  13;  Tate,  13; 
Thomson,  13 ;  Watson,  14. 

Analysis.    Barreswill  &  Sobrino,  1 ; 

Fresenius,  5 ;  Galloway,  5 ;  Gerhaldt,  6  ; 
Johnson,  7;  Liebig,  9;  Noad,10;  Normandy, 
10 ;  Parnell,  10  ;  Rose,  12  ;  Violette  et  Arch- 
ambault,  14 ;  Will  et  Liebig,  14 ;  Wohler,  14. 

Animal.    Berzelius,  2 ;  Thomson,  13. 

•  Appl  icd.    Ajasson  de  Grandsagne,  1 ; 

Annuaire  de  Chirnie,  1 ;  Barruel,  1 ;  Bernay, 
2,  Knapp,  3;  Daguin,  4  ;  Dumas,  5  ;  Fran- 
cceur,  5 ;  Graham,  6  ;  Kemp,  8 ;  Miahle,  9 ; 
Morflt,  10 ;  Muspratt,  10 ;  Parnell,  10 ;  Payen, 
10 ;  Thomson,  13. 


—  Catechism.    Graham,  6 ;  Horsley,  T. 

—  COUTH  et  Lecons.    Boutet  de  Mor- 
vel,2;  Cabai-t,8;  Gerhardt-,6;  Reguault, 


Chemistry,  Elements  of.  Graham,  6; 
Kane,  8 ;  Miller,  9  ;  Murray,  10 ;  Regnault, 
12 ;  Thomson,  13 ;  Turner,  14 ;  Weldon,  14. 

Elementary.  Cahours,  3 ;  Daguin, 

4;  Fyfe,  5;  Glover,  6;  Gregory,  6;  Mala- 
guiti,  9  ;  Regnault,  12 ;  Thenard,  13. 

First  Steps.    Galloway,  5. 

General.    Baudrimont,  1 ;  Berzelius, 

2;  Pelouze  &  Fremy,  11. 

Handbook.     Gmelin,  6. 

History.    Hoefer,  7 ;  Thomson,  13. 

Inorganic.     Campbell, 3;  Berzelius, 

2;  Gmelin,  6;  Gregory,  6;  Outlines  of,  7; 
Thomson,  13. 

Lectures.    Gurney,  6. 

Manual.    Bernay,  2 ;  Brande,  3 ; 

Fyfe,  5 ;  Glover,  6. 

Manipulation.  Faraday,  5 ;  Noad 

10;  Benoit. 

Memoirs.    Dumas,  5 ;  Graham,  6. 

Non-Metallic.     Faraday,  5. 

Organic.    Brande,  2 ;  Dumas,  5 ;  Ger- 

hardt,  6 ;  Gmelin,  6 ;  Gregory,  6  ;  Lowig,  9 ; 

Millon,    9;     Raspail,    12;     Thomson,    18; 

Wolff,  14. 

Philosophy.    Dalton,  4 ;  Daniell,  4 ; 

Davy,  4 ;  Webster,  14 ;  Weekes,  14. 
Practical.    Bowman,  2. 

Progress  off.      Berzelius,  2;  Liebig 

and  Kopp,  9. 

Treatise.    Gregory,  6. 

Crystallography.  Dcscloizeaux,4;  Lau 
rent,  8 ;  Regnault,  12. 

Colors  and.  Painting.  Chevreul,3;  Co- 
loriste,  4. 

Cyclopaedia.  Cooley,  4;  Francis,  5 ;  Pre- 
chtl,  11 ;  Thomson,  1 ;  Tomlinson,  13. 

Dictionary  (Chemical,  etc.)  Cheval- 
lier,  3 ;  Crabb,  4 ;  Hoefer,  7 ;  Laboulaye, 
8;  Lassaigne,  8;  Nesbit,  10;  Ottley.  10: 
Tollhausen,  13 ;  Ure,  14. 

Distilling.  Dubrunfaut,  5 ;  Duplais,  5 ;  La- 
cambre,  8 ;  Le  Normand,  9 ;  Morewood,  10. 

Dyeing  and  Scouring.  Berthollet,  2 ; 
Blanchiment,  2 ;  Brande,  2 ;  Love,  9  ;  Na 
pier,  10;  Parnel,  10 ;  Persoz.  11 :  Kunze,12 ; 
Smith,  13;  Thomson,  13. 


16 


Alphabetical  Index. 


Electricity.  Becquerel,  2;  Chalmers,  8; 
Gumming,  4 ;  De  la  Rive,  4 ;  De  Bois  Ray 
mond^;  Faraday,5;  Harris,  7 ;  Matteuci, 9; 
Murphy,  10  ;  Noad,  10. 

Electric- Telegraph.  Highton, 7 ; 
Moigno,  10. 

Electro-Metallurgy.  Dorure,  4;  Gal- 
vanoplastie,  5 ;  Gore,  6;  Napier,  10  ;  Rose- 
leur,  12 ;  Smee,  13  ;  Walker  et  Fau,  14. 

Falsifications.  Chevallier,  3 ;  Hassall,  7 ; 
Bureaux,  7 ;  Marcet,  9  ;  Mitchell,  10. 

Food.    See  Falsification*. 

Gas.  Accum,  1 ;  Clegg,  4 ;  Knapp,  8 ;  Journal 
of,  6 ;  Matthews,  9 ;  Peckston,  11 ;  Pelouze,  11. 

Geological  Chemistry.    Bischoff,  2. 

Glue.    Colles,  4. 

Heat.  Avogrado,  1 ;  Cooper,  4  ;  Dove,  6 ; 
Gavarret,  6  ;  Lardner,  8  ;  Metcalfe,  9  ;  Pe- 
clet,  11 ;  Poisson,  11 ;  Prideaux,  11  ;  Reech, 
12 ;  Regnault,  12 ;  Thomson,  13 ;  Williams,  14. 

Ink.    Encres,  4. 
Magnetism.    Becquerel,  2. 

Meteorology.  Arago,  1 ;  Cotte,  4 ;  Hop 
kins,  7  ;  Houzeau,  7  ;  Howard,  7 ;  Kaemtz,  8 ; 
Lambert,  8  ;  Nicollet,  10 ;  Peltier,  11 ;  Pouil- 
let.ll ;  Prout.ll ;  Robertson,  12 ;  Sabine,  12. 

Mineral  Waters.    Bouquet,  2 ;  Faure,  5. 


Optics  and  Light.     Biot,  2 ;  Brewster 
Claudet,  4 ;  Du  Moncel,  5 ;  Gorham,  6 ;  H 


Har 


dy,  7 ;  Hunt,  7  ;  Kyan,  8  ;  Light,  9 ;  Moigno, 
10 ;  Scantini,  12 ;  Scoffern,  18. 


Perfumery.    Piesse,  11. 

Pharmacy.  Deschamps, 
Guibourt,  6 ;  Jourdain,  8 ; 
Journal,  11 ;  R 
18;  Wittstein,: 


4;  Goebel,  6; 
Pharmaceutical 
Soubeiran, 


Pharmacopeia.  Codex,  4 ;  New  London, 
11 ;  Trousseau  and  Reveil,  14. 

Photography.  Barreswil  and  Davanne,  1 ; 
Blanquart,  2;  Brebisson,  8;  Chevallier,  3  ; 
Cundall,  4;  David,  4;  Delamotte,  4;  De- 
songe,  4;  Disderi,  4;  Fau,  5;  Gaudin,  6; 
Hardwicke,  7  ;  Heath,  7  ;  Hennah,  7  ;  Her- 
ling,  7;  Hewlett,  7;  Hunt,  7 ;  Lacan,  8 ; 
Legray,  8  ;  Lerebours,  9  ;  Long,  9  ;  Mar 
tens;  9  ;  Rintoul,  12 ;  Button,  13  ;  Thorn- 
thwaite,  13. 

Physics.  Aime  Martin,  1 ;  Ajasson  de 
Grandsagne,  1  ;  Archambault,  1 ;  Biot,  2 ; 
Bird,  2  ;  Boutigny,  2  ;  Brown,  3  ;  Cabart,  3  ; 
Coulomb,  4;  Cuvier,  4;  Daguin,4;Desains,4; 
Durand,  5 ;  Fau  and  Chevallier,  5 ;  Ganot,  5 ; 
Grove,  6;  Gruyer,  6;  Guitard,6,  Hinds,  7; 
Julien,  8 ;  Lame,  8 ;  Lardner,  8 ;  Liebig,  9 ; 
McGauley,  9;  Muller,  10;  Peclet,  11 ;  Pou- 
illet,  11 ;  Quetelet,  11 ;  Regnault,  12 ;  Reichen- 
bach,  12;  Scoffern,  13;  Scoresby,  13;  Sou 
beiran,  13 ;  Thieme,  13. 

Platina.    Billard,2. 

Polarization.  Bi«t,  2 ;  Pereira,  11 ;  Wood 
ward,  14. 

Precious  Metals.    Faucher,  5. 
Pyrotechny.    Chertier,  8. 

Rural  Economy.  Bouchardat,  2 ;  Bous- 
singault,  2. 

Safety  I>amps  for  Miners.    Davy,  4 ; 

Knapp,  8. 

Sugar.  Baudrimont,  2  ;  Kerr,  8 ;  Scoffern,  13 ; 
Shier,  13. 

Ventilation.  Arnott,  1 ;  Dunn,  5  ;  Hed- 
ley,  7;  Hood,  7;  Mather,  8;  Reid,  12; 
Richardson,  12. 

Weaving:.   Etoffes  Imprimees,  5 ;  Person,  11. 


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